Saturday
April 19, 2014

Search: calculate Kp for the reaction below. 1/2CH3OH <>1/2CO + H2

Number of results: 49,288

Chemistry 2
Calculate Kp for the reaction C(s)+CO2(g)<-->2CO(g) kp=? C(s)+2H2O(g)<--->CO2(g)+2H2 kp1=3.47 H2(g)+CO2(g)<--->H2O(g)+CO(g) kp2=0.735
Friday, February 21, 2014 at 1:30pm by Sharon

Chemistry
Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to from nitric acid. One of the possible reactions is shown below. Calculate ∆G0 and Kp for this reaction at 25oC and comment of on the spontaneity of the reaction (MUST plot the data and find ...
Thursday, April 18, 2013 at 11:02am by Yasemine

Chemsitry
Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to from nitric acid. One of the possible reactions is shown below. Calculate ∆G0 and Kp for this reaction at 25oC and comment of on the spontaneity of the reaction (MUST plot the data and find ...
Friday, April 19, 2013 at 11:32am by Yasemine

CHemistry
CH4(g) + CO2(g) <--> 2CO(g) + 2H2(g) Kp = 4.5 x 10^2 at 825 K An 85.0 L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. Assuming ideal gas behavior, calculate the mass of H2 present in the reaction mixture at equilibrium.
Thursday, March 18, 2010 at 9:34pm by Krysten

chemistry
Kp for the reaction is 1.47 at 727S CO2(g) + C(s) 2CO(g) Calculate Kc at this temperature
Saturday, July 21, 2012 at 11:12pm by ken

college
Kp for the reaction CO2(g) + C(s) 2CO(g) is 1.47 at 727C. Calculate Kc at this temperature
Sunday, July 22, 2012 at 11:20pm by gggg

chemistry
Determine Kc at 298 K for the reaction 2 CH4(g) reverse reaction arrow C2H2(g) + 3 H2(g), given the following data at 298 K. (Hint: How are Kc and Kp for the reaction related?) CH4(g) + H2O(g) reverse reaction arrow CO(g) + 3 H2(g) Kp = 1.2 multiplied by 10-25 2 C2H2(g) + 3 O2...
Wednesday, March 24, 2010 at 6:21pm by Jenny

Chemistry
In the gas phase reaction CH4 + H2O → CO + 3 H2 At T = 1500 K , Kp = 11000 Calculate Kp, T = 1500 K , for the following reaction 3 CO + 9 H2 → 3 CH4 + 3 H2O .
Thursday, September 24, 2009 at 1:35pm by Ava

Chemistry/Equilibrium calculations
2CO2(g) <=> 2CO(g)+ O2(g) Kp = 1 E-13 (or 1.00x10^-22) The LEFT side is favored. It is perfectly proper to write the reaction backwards: 2CO(g)+ O2(g) <=> 2CO2(g) BUT now the Kp is the reciprocal of 1.00x10^-22 or Kp = 1.00x10^22 for the reversed reaction The above...
Saturday, August 16, 2008 at 7:59am by GK

Chemistry
Calculate the value of Kp for the equation C(s)+CO2(g)<->2CO(g) Kp=? given that at a certain temperature C(s)+2H2O(g)<->CO2(g)+2H2(g) Kp1=3.33 H2(g)+CO2(g)<->H2O(g)+CO(g) Kp2=.733 Please show detailed steps.
Thursday, February 7, 2013 at 8:27pm by Julia

Chemistry
What is the value of Kp for the reaction: NO2(g)+CO(g)->NO(g)+CO2(g) Given the following information: 2NO2(g)->NO3(g)+NO(g) Kp=2.72x10^(-4) 2NO2(g)+2CO2(g)->2NO3(g)+2CO(g) Kp=5.73
Sunday, November 27, 2011 at 10:09pm by Tanya

Ap Chem
Consider the following reaction at 1000C:CO(g) + 3H2(g) CH4(g)+ H2O(g) At equilibrium, the following concentrations are measured: [CO] = 0.0613 M, [H2] = 0.1839 M, [CH4] = 0.0387, [H2O] = 0.0387 M. Calculate the value of Kc for this reaction. Calculate the value of Kp. Ans.: ...
Sunday, October 9, 2011 at 10:47am by Jane

college chemistry
Methane reacts with water to form CO and H2 as follows CH4 (g) + H2O (g) >< CO (g) + 3 H2 (g) The value of Kp at 298 K for the reaction is 7.7 x 1024, calculate Kc.
Thursday, September 30, 2010 at 10:11am by mary

Chem12
Calculate Kp for the reaction N2(g) + 3 H2(g)--> 2 NH3(g) given that the reaction has Kc = 438,880,639 at a temperature of 265.
Monday, May 2, 2011 at 11:47pm by Ryan

chemistry
Kp for the reaction CO2(g) + C(s) 2CO(g) is 1.47 at 727C. Calculate Kc at this temperature Answer A. 0.0179 B. 0.0246 C. 121 D. 87.7 E. 1.47
Saturday, July 21, 2012 at 11:22pm by ken

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) My Answer: To find the reverse reaction of Kc, it should be 1/0.2 = 5, so the ...
Sunday, March 18, 2012 at 10:16pm by Raskin

Chemistry
If someone could please be kind enough to see me through this problem? Calculate the value of Kp for the equation C(s) + CO2(g) <--> 2CO(g) Kp? Given that at a certain temperature.. C(s) + 2H2O(g) <--> CO2(g) + 2H2(g) Kp1 = 3.03 and H2(g) + CO2(g) <--> H2O(g...
Monday, March 5, 2012 at 10:14pm by Tracy

Chemistry
A container is filled with CO2(g) and heated to 1000K. The gas pressure at this temperature is 0.50 atm. Graphite (C) is then added to the container and some of the CO2 is converted to CO according to the reaction below. The final equilibrium total gas pressure in the flask is...
Wednesday, July 24, 2013 at 9:01am by Nat

Chemistry
A 0.960mol quantity of Br2 is added to a 1.00 L reaction vessel that contains 1.23mol of H2 gas at 1000 K. What are the partial pressures of H2, Br2, and HBr at equilibrium? At 1000 K, Kp=2.1106 and ΔH∘ = -101.7 kJ for the reaction H2(g)+Br2(g)⇌2HBr(g).
Monday, February 3, 2014 at 9:58pm by Myles Tan

Chemistry
For the following reaction, Kp = 3.5 104 at 1495 K. H2(g) + Br2(g) 2 HBr(g) What is the value of Kp for the following reactions at 1495 K? (a) HBr(g) 1/2 H2(g) + 1/2 Br2(g) (b) 2 HBr(g) H2(g) + Br2(g) (c) 1/2 H2(g) + 1/2 Br2(g) HBr(g)
Monday, February 20, 2012 at 9:10pm by Elizabeth

chemistry
Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g)
Friday, April 2, 2010 at 11:02pm by bme1

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) I'm sorry.. English is a second language for me. After solving for K'c and ...
Thursday, March 15, 2012 at 9:55pm by David

Chem
For each unbalanced equation below, calculate how many grams of each product would be produced by complete reaction of 12.5g of the reactant indicated. Indicate clearly the mole ratio used for the conversion. A. TiBr4(g)+H2(g)=Ti(s)+HBr(g), Reactant is H2 B. SiH4(g)+NH3(g)=...
Wednesday, June 25, 2008 at 2:59pm by OliviaK

Chemistry
If the reaction Fe2N(s) + 3/2H2(g) -> 2Fe(s) +NH3(g) comes to equilibrium at a total pressure of 1 bar, analysis of the gas shows that at 700. and 800.K, PNH3/PH2=2.165 and 1.083 respectively, if only H2(g) was initially present in the gas phase and Fe2N(s) was in excess. a...
Tuesday, November 23, 2010 at 1:22am by Katie

chemistry
A 0.100 mol sample of H2S is placed in a 10.0 L reaction vessel and heated to 1132C. At equilibrium, 0.0285 mol H2 is present. Calculate the value of Kc for the reaction below at 1132C. 2 H2S(g) 2 H2(g) + S2(g)
Monday, January 31, 2011 at 10:38pm by Brittany

Chem
Which direction will the following reaction in a 5.0 L flask proceed if Qp = 0.013? 2H2O(g) = 2H2(g) + O2(g) Kp = 1.6 x 10-5 Choose one answer. a. to the right because Q > Kp b. to the left because Q > Kp c. to the right because Q < Kp d. to the left because Q < Kp...
Wednesday, March 24, 2010 at 11:28pm by CC

chemistry
Calculate the value of the equilibrium constant, Kp , for the following reaction at 298.0 Kelvin. (Use the reaction free energy given below.) 2SO3 = 2SO2 + O2 in the gaseous state ΔG = 140.0 kJ/mol
Tuesday, October 12, 2010 at 10:46pm by lizz

chemistry
Calculate the value of the equilibrium constant, Kp , for the following reaction at 298.0 Kelvin. (Use the reaction free energy given below.) 2SO3 = 2SO2 + O2 in the gaseous state ΔG = 140.0 kJ/mol
Tuesday, October 12, 2010 at 10:47pm by lizz

Chemistry
A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800C. Calculate the equilibrium partial pressures of H2 Cl2 and HCl if the total pressure is 2.00 atm. For the reaction Kp is 193 at 2800C. H2(g) +Cl2(g) = 2HCl (g) I know that I need to find the total numbers of...
Saturday, October 16, 2010 at 8:51pm by Ashley

Chemistry
Calculate the enthalpy change for the reaction 2C + H2 yield C2H2 given the following reactions and their respective enthalpy changes: C2H2 + 5/2 O2 yield 2CO + H2O -1299.6 C + O yield CO2 -393.5 H2 + 1/2 O2 yield H2O -285.9 I don't even know how to start and the example in ...
Monday, December 24, 2007 at 5:28pm by Lucy

chemistry
For the reaction shown below complete the following calculations. H2(g) + C2H4(g) --> C2H6(g) (a) Estimate the enthalpy of reaction using the bond energy values in Table 9.4. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (ΔHf for H2, ...
Monday, October 27, 2008 at 11:24pm by hannah

chemistry
at 327 degrees C, the equilibrium concentrations are [CH3OH]=0.15M, [CO]=0.24M, and [H2]=1.1M for the reaction: CH3OH(g)<-->CO(g)+2H2(g) Calculate Kp at this temperature
Wednesday, February 16, 2011 at 8:24pm by erica

Chem!!
The value of H for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO(g) reacts completely. 2CO(g) + O2(g) 2CO2(g)
Wednesday, June 6, 2012 at 2:39pm by Harlem

Chemistry
At 389K, this reaction has a Kc value of 0.0682. 2X(g) + 2Y(g) <-> Z(g) .. Calculate Kp at 389K. Kp= this is what I did.. can somebody confirm or find any mistakes in my thought process? Kp = Kc(R)(T)^Delta n Delta n = (1)-(2+2) = -3 Kp = (0.0682)(0.08206)(398K)^-3 = 0....
Monday, March 5, 2012 at 8:35pm by Tracy

chemistry
The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely. 2CO(g) + O2(g) --> 2CO2(g)
Monday, April 16, 2012 at 11:11am by tank

chemistry
The dH for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely. 2CO(g) + O2(g) --> 2CO2(g)
Monday, April 16, 2012 at 11:11am by tank

Chemistry
The problem gives you the Kp at 400 C. We presume the reaction is at the same temperature as Kp is given Kp = pNH3*pHI NH4I(s) ==> NH3(g) + HI(g) ..............p.......p Substitute p into Kp expression and solve for p.
Thursday, March 8, 2012 at 7:42pm by DrBob222

chem
If the initial pressure of HD(g) is 2.270 atm, calculate the % decomposition of HD(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 727.0 C is 0.26. The initial pressure of the reaction products is 0 atm. 2HD(g) = H2(g)+D2(g)
Friday, September 30, 2011 at 5:51pm by BOB

Chem14
The reaction 2 H2S(g)--> 2 H2(g) + S2(g) has Kp = 2.4 x 10-4 at 1073 K. A reaction mixture contains 0.146 atm of H2, 0.041 atm of S2 and 0.574 atm of H2S. What is the value of Qp?
Monday, May 2, 2011 at 11:49pm by Ryan

Chemistry
At 400C the reaction H2+I2<->2HI has an equilibrium constant Kp value of 55.5. A mixture of 1 mole of H2 and 1 mole of I2 is placed in a flask and heated to 400C. Calculate the mole fraction of HI in the mixture of gases when equilibrium reached.
Friday, February 1, 2013 at 6:00pm by Kelly

Chemistry
One mole of N2 and three moles of H2 are placed in a flask at 375 C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31*10^4. I assume this to be the reaction N2 + 3H2 --> 2NH3 Help ? Forgot to ...
Wednesday, March 2, 2011 at 8:44pm by Chemmy

Chemistry
One mole of N2 and three moles of H2 are placed in a flask at 375 C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31*10^4. I assume this to be the reaction N2 + 3H2 --> 2NH3 Help ? Forgot to ...
Wednesday, March 2, 2011 at 8:44pm by Chemmy

chemistry(check my work)
Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g) is it like this, (5.462)^2/(0.2282x0....
Sunday, April 4, 2010 at 6:24pm by bme1

Chemistry
consider the following reaction: 2CH3OH(g) yields 2CH4(g) + O2(g) change in enthalpy= 252.8kJ Calculate the amount of heat transferred when 26.0 g of {\rm CH_3OH} (g) is decomposed by this reaction at constant pressure.
Monday, March 5, 2012 at 6:51pm by Dylan

chemistry
At 850 K, the value of the equilibrium constant Kp for the ammonia synthesis reaction N2(g) + H2(g) <--> N2H2(g) is 0.1690. If a vessel contains an initial reaction mixture in which [N2]=0.0150 M, [H2]=0.0200 M, and [N2H2]=0.000250 M, what will the [N2H2] be when ...
Monday, November 5, 2012 at 11:24am by Victoria

Chemistry
C(s)+2H2O(g)<->CO2(g)+2H2(g) Kp1=3.33 H2(g)+CO2(g)<->H2O(g)+CO(g) Kp2=.733 Multiply equation 2 by 2 and add to equation 1 to obtain: C(s) + 2H2O + 2H2 + 2CO2 ==> CO2 + 2H2 + 2H2O + 2CO Notice 2H2O cancels, 2H2 cancels, 1 CO2 cancels to leave C(s) + CO2 ==> ...
Thursday, February 7, 2013 at 8:27pm by DrBob222

chemistry
Posted a question earlier but it was the wrong question. If anyone could help it would great if you could explain this would help also. Thanks ^ = subscript Calculate ke for(equlibrium concentration below problem 2CO^2(g) + heat 2CO(g) + O^2 [0.103] [0.024] [1.18 x 10^2]
Tuesday, January 5, 2010 at 12:47pm by Shanta

Chemistry
Methane reacts with water to form CO and H2 as follows: CH4(g)+H2O(g)=CO9g)+3H2(g) The value of Kp at 298 k for the reaction is 7.7 *10^24, calculate Kc. If you can please show the steps I would greatly appreciate it. Thank you
Tuesday, December 10, 2013 at 4:06am by craig

Chemistry
A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800C. Calculate the equilibrium partial pressures of H2 Cl2 and HCl if the total pressure is 2.00 atm. For the reaction Kp is 193 at 2800C. H2(g) +Cl2(g) = 2HCl (g) What I've done so far: found the partial ...
Sunday, December 19, 2010 at 11:38am by Jamal

Chemistry
Consider the reaction below. 3 O2(g) --> 2 O3(g) At 175C and a pressure of 128 torr, an equilibrium mixture of O2 and O3 has a density of 0.168 g/L. Calculate the Kp for the above reaction of 175C
Monday, February 20, 2012 at 9:15pm by Elizabeth

Chemistry
Consider the reaction below. 3 O2(g) --> 2 O3(g) At 175C and a pressure of 128 torr, an equilibrium mixture of O2 and O3 has a density of 0.168 g/L. Calculate the Kp for the above reaction of 175C
Monday, February 20, 2012 at 11:46pm by Andre

Chemistry
At 1200 K, the approximate temperature of vehicle exhaust gases, Kp for the reaction 2CO2(g)⇄2CO(g) + O2(g) is about 1*E-13. Assuming that the exhaust gas (total pressure 1 bar) contains 0.2% CO, 12% CO2 and 3% O2 by volume, is the system at equilibrium with respect to ...
Saturday, August 16, 2008 at 6:35am by Helen

Chem
The value of H for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO(g) reacts completely. 2CO(g) + O2(g) 2CO2(g) *I just want to how to solve this problem as in an equation, not the answer. thank you!
Friday, June 8, 2012 at 3:03pm by Harlem

Intro Chemistry
Are you assuming that the reaction goes to completion? You don't have a Kp or Kc listed. What's the limiting reagent? I believe that is CO. ............2CO + O2 ==> 2CO2 I...........10....8........0 C..........-10...-5.......10 E...........0.....3.......10 So you have 13 ...
Sunday, May 5, 2013 at 1:08pm by DrBob222

AP CHEM!
IM SO CONFUSED PLEASE HELP! H2 +CO2-->H2O + CO When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured. [H2]= 0.20mol/L [CO2]= 0.30mol/L [H2O]=[CO]= 0.55mol/L a/ ...
Tuesday, April 3, 2007 at 10:07pm by linds

Idontgetit
The value of the equilibrium constant (Kp) as represented by the first chemical equation is 2.00 x 10-2 at 730 K. Calculate the value of the equilibrium constant (Kp) for the second equation at the same temperature. Express answer in scientific notation. 2HI(g) = H2(g)+I2(g) ...
Wednesday, October 2, 2013 at 3:43pm by Chemistry

Chemistry (please help me!)
H2(g) + CO2(g)<-> H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M [H2O]=[CO]=0.55M a) What is the mole ...
Sunday, February 25, 2007 at 6:07pm by sara

Chemistry
At 1200 K, the approximate temperature of vehicle exhaust gases, Kp for the reaction <- 2CO2(g) -> 2CO(g) + O2(g) is about 1*10E-13. Assuming that the exhaust gas (total pressure 1 bar) contains 0.2% CO, 12% CO2 and 3% O2 by volume, is the system at equilibrium with ...
Saturday, August 16, 2008 at 6:31am by Helen

AP Chemistry
The equilibrium constant Kp is 5.0010^17 at 25◦C for the reaction C2H4(g) + H2(g)<->C2H6(g). From this information, calculate ∆G0 at 25◦C
Tuesday, November 26, 2013 at 7:52pm by Gabriella

Chemistry
The value of Kc for the reaction below is 1.6 C(s)+CO2(g)=2CO(g) What is the equilibrium concentration of CO when [CO2]=.50M? The usual ICE table doesn't work for me. C(s)+CO2(g)=2CO(g) I - 0 C -x +2x E .50 +2x 1.6=[2x]^(2)/(.50) That's how I did it but the answer is .89 and I...
Friday, March 22, 2013 at 12:42pm by Ezra

chemistry
I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the equilibrium constant (...
Thursday, April 8, 2010 at 5:20pm by andy

chemistry
Calculate the mass of co2 produced when 2ch3oh mixed with o2. Given that 2ch3oh is 4o grams and o2 is 46 grams.
Tuesday, April 9, 2013 at 12:42pm by Ruusa

chemistry
Calculate the mass of co2 produced when 2ch3oh mixed with o2. Given that 2ch3oh is 4o grams and o2 is 46 grams.
Tuesday, April 9, 2013 at 12:53pm by Ruusa

Chemistry (Equilibrium)
Given the reaction below 2NOBr(g) <==> 2NO(g) + Br2(g) and the value of Kc = 1.98, at a temperature of 480 K what is the value of Kp ? (Hint: Use the value of R in the appropriate units.) I used the equation Kp=Kc(RT)^Delta N Then plugged in to get Kp=1.98(.0821x480k)^-1...
Friday, December 9, 2011 at 7:46pm by Summer

Chemistry
A 893 g sample of a solution of the solute (CH3)2CO in the solvent C4H8O that has a concentration of 28.6 pph by mass (CH3)2CO is available. Calculate the amount (g) of acetone that is present in the sample. Molar Mass (g/mol) (CH3)2CO 58.05 C4H8O 72.12 Density (kg/m3): (CH3)...
Sunday, February 14, 2010 at 9:20pm by Anonymous

FlunkyJunkie
Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100. g solution. Molar Mass (g/mol) (CH3)2CO 58.05 H2O 18.015 Density (g/mL): (CH3)2CO 0.7899 H2O 0.9982 ...
Sunday, February 14, 2010 at 9:30pm by Jackie

chemistry
Calculate the volume (mL) of the solute (CH3)2CO and the volume (L) of the solvent H2O that should be added to prepare 1.36 kg of a solution that is 25.7 g (CH3)2CO per 100. g solution. Molar Mass (g/mol) (CH3)2CO 58.05 H2O 18.015 Density (g/mL): (CH3)2CO 0.7899 H2O 0.9982 ...
Sunday, February 14, 2010 at 9:36pm by Jackie

Chemistry
When 0.59 mol I2(g) and 0.59 mol H2(g) are placed into a 1.0-L container at a given temperature, 0.30 mol H2(g) is found to be present after the reaction below reaches equilibrium. Calculate Kc at the given temperature. I2(g) + H2(g) 2HI(g)
Friday, November 19, 2010 at 10:00pm by Shayne

Chem 2
need to figure out how to calculate. the value of DeltaH for the reaction below is -72kj_____kj of heat are released when 1.0 mole of HBr is formed in this reaction. H2(g)*Br2(g)> 2HBr(g) I know the answer is 36 but need help
Friday, March 30, 2012 at 3:14pm by Debbie

Chemistry
Nitrogen Dioxide , a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possible reactions is shown here. Calculate delta ∆G and Kp for this reaction at 25C and comment on the spontaneity of the reaction. 3NO2(g)+H2O(l)--> 2 HNO3(aq...
Thursday, March 29, 2012 at 4:40pm by SANDY

Chemistry/Equilibrium calculations
At 1200 K, the approximate temperature of vehicle exhaust gases, Kp for the reaction 2CO2(g)-> <- 2CO(g)+ O2(g) is about 1 E-13. Assuming that the exhaust gas (total pressure 1 bar) contains 0.2% CO, 12% CO2 and 3% O2 by volume, is the system at equilibrium with respect ...
Saturday, August 16, 2008 at 7:59am by Mary

Chemistry
The equilibrium constant for the reaction 2NO(g) + O2(g) <--> 2NO2(g) is Kp=1.48x10^4 at 184C. Calculate Kp for 2NO2(g) <--> 2NO(g) + O2(g). I know the equation is Kp=Kc(RT)x Delta n Kp is what we're solving for Kc= I can't seem to find. R=.0821 T=184+273 Delta n= ...
Tuesday, March 9, 2010 at 5:06pm by Anonymous

chemistry
A 893 g sample of a solution of the solute (CH3)2CO in the solvent C4H8O that has a concentration of 28.6 pph(parts per hundred) by mass (CH3)2CO is available. Calculate the amount (g) of acetone that is present in the sample. Molar Mass (g/mol) (CH3)2CO 58.05 C4H8O 72.12 ...
Tuesday, February 16, 2010 at 7:03pm by Angel

Chemistry
8. For the reaction H2(g)+I2(g)\2HI(g); [H2] = 0.95 M; [I2] = 0.78 M; [HI] = 0.27 M. Calculate the equilibrium constant K and describe the direction (forward or reverse) of the reaction. Will adding a catalyst to the reaction alter the direction of the reaction? Why? Describe...
Monday, March 29, 2010 at 11:48am by Kathleen

Chemistry
Consider the reaction: 2 H2S(g)--><-- 2H2(g) + S2 Kp= 2.4 x 10^-4 at 1073k A reaction mixture contains .112 atm of H2,.055 atm of S2, and .445 atm of H2S. Is the reaction mixture at equlibrium? If not, in what direction will the reaction proceed?
Wednesday, February 23, 2011 at 1:42pm by sally

Chemistry
Consider the reaction: 2 H2S(g)--><-- 2H2(g) + S2 Kp= 2.4 x 10^-4 at 1073k A reaction mixture contains .112 atm of H2,.055 atm of S2, and .445 atm of H2S. Is the reaction mixture at equlibrium? If not, in what direction will the reaction proceed?
Wednesday, February 23, 2011 at 1:42pm by sally

Chemistry
MF17083:For the following reaction find Kp at 25C and indicate whether Kp should increase or decrease as the temperature rises. NH4HS(s) <===> H2S(g) + NH3(g); DH = 83.47 kJ and DG = 17.5 kJ at 25C. - A. B. C. D. E. F. Kp = - A. B. C. D. E. F. Kp ________ as the ...
Friday, April 27, 2007 at 12:52pm by Chris

Dan
or mike or whomever, Two points: 1. How do you know to calculate Kc instead of Kp? The problem doesn't specify which. Since this is a gaseous reaction, Kp may be what they are looking for. 2. Have you tried the van't Hoff equation. You have delta H and one T so the van't Hoff ...
Saturday, November 17, 2007 at 1:06pm by DrBob222

chemistry
2. Methanol, CH3OH, is used as fuel in race cars. This liquid fuel can be synthesized using the following process C(s)+ O2(g) + 2H2(g)  CH3OH(l) Calculate delta G using the deta Gf of the reaction. Calculate Kp. What is the relation between the magnitude of delta G ...
Thursday, April 15, 2010 at 7:32am by Kristen

Chemistry
You are given the following decomposition reaction of ammonia NH3 ---> H2 + N3 unbalanced When you decompose 12.0g of NH3you produce 1.87 g of H2 Calculate the percent yield of H2
Thursday, April 18, 2013 at 2:07am by Johny

chemistry
start with the equation for the reaction 2Al + 6H2O --> 2Al3+ + 3H2(g) + 6OH- This is because the OH- removes the oxide coating from the Al, but the reaction is with the water. Hence we can see that 2 moles of Al yields 3 moles of H2. From your volume of H2 (you also need ...
Thursday, November 25, 2010 at 4:18am by Dr Russ

Chem
At 850 C, the equilibrium constant Kp for the reaction: C(s)+CO2(g) >< 2CO(g) has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide.
Wednesday, April 22, 2009 at 2:01pm by Noemi

chemistry
please help and explain. At a certain temperature, Keq = 10.5 for the equilibrium below. CO(g) + 2 H2(g) equilibrium reaction arrow CH3OH(g) Calculate the following concentrations. (b) [H2] in an equilibrium mixture containing 1.01 mol/L CO and 0.335 mol/L CH3OH
Monday, March 11, 2013 at 3:46pm by Julia

Chemistry
Consider the reaction: 2CO2(g)=2CO(g) + O2(g). A reaction mixture in a 5.0 L flask at a certain temperature. At equilibrium there are 85 g of CO2(g), 1.20 g of CO, and 0.688 g of O2(g). Calculate Kc.
Sunday, February 27, 2011 at 11:51pm by Ariel

Chemistry
Consider the reaction: 2CO2(g)=2CO(g) + O2(g). A reaction mixture in a 5.0 L flask at a certain temperature. At equilibrium there are 85 g of CO2(g), 1.20 g of CO, and 0.688 g of O2(g). Calculate Kc.
Sunday, February 27, 2011 at 11:52pm by Ariel

Chemistry
Consider the reaction: 2CO2(g)=2CO(g) + O2(g). A reaction mixture in a 5.0 L flask at a certain temperature. At equilibrium there are 85 g of CO2(g), 1.20 g of CO, and 0.688 g of O2(g). Calculate Kc.
Sunday, February 27, 2011 at 11:52pm by Ariel

chemistry
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K. Do you expect Kp to increase or decrease as the temperature is increased to 600 K?
Sunday, April 7, 2013 at 5:49pm by hayley

chemistry
Calculate Kp at 298 K and 490 K for the reaction NO(g) + 1/2 O2(g) = NO2(g) assuming that Delta H(g) is constant over the interval 298 K - 600 K. Do you expect Kp to increase or decrease as the temperature is increased to 600 K?
Sunday, April 7, 2013 at 5:49pm by ahsang

chemistry
The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. Calculate Kc for this reaction at this temperature. 2SO3(g) 2SO2(g) + O2(g)
Sunday, March 9, 2014 at 2:52pm by Anonymous

chemistry
CO2(g) + H2(g) equilibrium reaction arrow CO(g) + H2O(g) Calculate the equilibrium concentration of each compound if 2.00 moles of CO2 and 2.40 moles of H2 are placed in a 3.90 liter container at 300C. Kc = 2.30 for the reaction at this temperature. [CO2] = M [H2] = M [CO] = ...
Wednesday, December 18, 2013 at 9:36pm by Isaiah

Chemistry(Please respond, thank you!)
For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction? Kp would = CaCO3/(CaO)(CO2) I do not know what to do with the 0.500M and 1.00mol. Chemistry...
Thursday, March 15, 2012 at 1:02pm by Hannah

Chemistry
initial pressure NH3 = 0.7317 atm. initial pressure H2 = 0 and N2 = 0 At equilibrium N2 = x H2 = 3x NH3 = 0.7317 - 2x Kp = 67,100 = pN2*pH2^3/pNH3^2 Substitute into Kp and solve for x, then convert to NH3, H2, N2. Finally, pNH3 remaining (from above) to percent of original ...
Sunday, October 3, 2010 at 9:14pm by DrBob222

chemistry
The water gas shift reaction used commercially to produce H2(g): CO (g)+ H2O (g) --> CO2 (g) + H2(g). DeltaH=-41.2 kJ/mol Delta S= -42.1 J/mol*K Delta G= -28.6 kJ\mol Determine Kp at 850 K
Sunday, December 2, 2012 at 11:13am by Allyx3

Chemistry - Kp
What is the Kp for the following reaction: 2NH3(g) --> N2(g) + 3H2(g) This reaction is contained in 1.0 L container at 1,000 K and has reached equilibrium. (Kc = 4.0 x 10^-2). You have initially added 1,220 moles of NH3(g) in the flask.
Sunday, April 29, 2012 at 8:00pm by Addyson

Chemistry - Kp
What is the Kp for the following reaction: 2NH3(g) --> N2(g) + 3H2(g) This reaction is contained in 1.0 L container at 1,000 K and has reached equilibrium. (Kc = 4.0 x 10^-2). You have initially added 1,220 moles of NH3(g) in the flask.
Sunday, April 29, 2012 at 8:29pm by Addyson

Chemistry
A gas-phase reaction has Kp = 2.44 10 20 at 25 ◦ C. Calculate ∆G 0 for this reaction. Answer in units of kJ/mol rxn
Sunday, October 14, 2012 at 3:08pm by sam

Chemistry
Given the following reaction at equilibrium, if Kc = 1.90 x 1019 at 25.0 C, Kp = __________. H2 (g) + Br2 (g) ↔ 2 HBr (g)
Saturday, November 17, 2012 at 1:02am by Josh G.

chemistry
A 0.286g sample of Zn was used to produce H2(g)by the reaction. Zn(s)+ 2HCl(aq)> ZnCl2(aq) + H2(g) The barometric pressure was recorded as 761.6mm Hg and room temperature was 20degreesC. When the water levels of the eudiometer tube and graduated cylinder were equal, the ...
Monday, December 3, 2012 at 9:58pm by joann

Chemistry
Is that Kp in bar? ........C3H8 ==> C3H6 + H2 Total P = 2 = pC3H6 + pH2 + pC3H8 Solve for pC3H8 = 2-p-p = 2-2p Kp = p*p/(2-2p) Solve for p = H2 = C3H6
Friday, February 14, 2014 at 3:25pm by DrBob222

Chemistry
A 1.00-kg sample of Sb2S3(s) and a 10.0-g sample of H2(g) are allowed to react in a 25.0-L container at 713 K. At equilibrium, 72.6 g H2S(g) is present. What is the value of Kp at 713 K for this reaction? Sb2S3(s) + 3 H2(g) <----> 2Sb(s) + 3 H2S(g)
Wednesday, October 27, 2010 at 3:23pm by Shanice

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