2CO + H2

Number of results: 42,430

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
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

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. 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 ...
Sunday, March 18, 2012 at 10:16pm by Raskin

Chemistry
The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. 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&#...
Thursday, March 15, 2012 at 9:55pm by David

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 ...
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 10:47pm by lizz

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...
Monday, March 5, 2012 at 8:35pm by Tracy

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

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

Ap Chem
Consider the following reaction at 1000°C: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. ...
Sunday, October 9, 2011 at 10:47am by Jane

Chemistry
Consider the reaction below. 3 O2(g) --> 2 O3(g) At 175°C 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 175°C
Monday, February 20, 2012 at 11:46pm by Andre

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(....
Friday, December 9, 2011 at 7:46pm by Summer

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
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
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 25°C and comment on the spontaneity of the reaction. 3NO2(g)+H2O(l)--&...
Thursday, March 29, 2012 at 4:40pm by SANDY

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=....
Tuesday, March 9, 2010 at 5:06pm by Anonymous

chemistry
2. Methanol, CH3OH, is used as fuel in race cars. This liquid fuel can be synthesized using the following process C(s)+ ½ 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 ...
Thursday, April 15, 2010 at 7:32am by Kristen

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...
Saturday, November 17, 2007 at 1:06pm by DrBob222

Chemistry
MF17083:For the following reaction find Kp at 25°C 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 25°C. - A. B. C. D. E. F. Kp = - A. B. C. D. E. F...
Friday, April 27, 2007 at 12:52pm by Chris

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
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
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

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(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 - 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

Chem Check
Consider the following gas phase reaction: 3A(g)+ 2B(g) <==> 1C(g)+4D(g). At 181.1C, Kp=270.91. Calculate Kc under these conditions. My answer: change of n = (1+4)-(3+2)=0 kp=kc(RT)^(change of of n) 207.91=kc(.0821)(454.1)^0 Therefore, kc=270.91 Is this correct? ...
Friday, February 9, 2007 at 9:13am by Marisol

Chemistry
In which direction will the net reaction proceed. X(g) + Y(g) <==> Z(g) .. Kp = 1.00 at 300k for each of these sets of initial conditions? 1) [X] = [Y] = [Z] = 1.0 M a] net reaction goes to the left [this one?] b] net reaction goes to the right c] reaction is at ...
Monday, March 5, 2012 at 10:03pm by Tracy

chemistry
At a certain temperature, 514, Kp for the reaction, Cl2(g) + Br2(g) <=> 2 BrCl(g), is 6.98 x 107. Calculate the value of DGo in kJ for the reaction at 514 K.
Sunday, April 24, 2011 at 3:10pm by sam

Chemistry
A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.54 atm at 425 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the actual pressure in the flask was found to be 0.85 atm. Calculate Kp for the decomposition ...
Wednesday, February 13, 2013 at 7:09pm by Margaret

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

Chemistry(Please help)
First you need to work on the Kp expression. SOLIDS aren't used (pure liquids aren't either) so the expression is 1/pCO2 = Kp. The problem tells you that AT EQUILIBRIUM [CO2] = 0.150M. I would calculate Kc from Kc = 1/([CO2] then convert to Kp by Kp = Kc(RT)Dn
Wednesday, March 14, 2012 at 9:51pm by DrBob222

chm152
You still didn't say "of what" but I assume it is Kp after you filled in th remainder of the missing information. First you turned the reaction around. Let's designate the original Kp as Kp1. That makes the new Kp (which we will call Kp2) = 1/Kp1. THEN you ...
Saturday, March 27, 2010 at 11:25am by DrBob222

Chemistry
Calculate Kp at 298K for the reaction SO2 + NO2--->SO3 + NO
Wednesday, May 1, 2013 at 11:30am by Charlie

Chemistry practice
2CH3OH + 3O2 ==> 2CO2 + 4H2O DHrxn = (n*DHfproducts) - (n*DHfreactants). Look up delta Hf for CO2 and H2O and CH3OH, substitute into the equation I gave you above and calculate delta H for the reaction.
Sunday, July 31, 2011 at 1:50pm by DrBob222

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 ...
Tuesday, November 23, 2010 at 1:22am by Katie

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

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

equilibrium constant (Kp)
What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) --><-- 4 PCL3(l) Given the following at 200 C P4(s)+ 10 Cl2(g) --><-- 4 PCl5(s) Kc=8.12 PCl3(l)+ Cl2(g) --><-- PCl5(s) Kc=0.771 Answer: 6...
Wednesday, July 20, 2011 at 3:10pm by k

Chemistry
I converted Kp to Kc also but didn't arrive at the same answer. I think your Kc = Kp(RT)^-delta n is correct. But delta n is 1-2 = -1 so Kc = Kp(RT)^(-)(-1). and that makes Kc about 25. Check me out on that. (Z)/(X)(Y) and Q = 1 which is too small so the reaction will ...
Monday, March 5, 2012 at 10:03pm by DrBob222

chemistry
At 25C, Kc= 3.7x10^9 for the reaction CO(g) + Cl2(g) equilibrium with COCl2(g) Calculate the Kp at this temperature.
Tuesday, October 9, 2007 at 7:52pm by Wolf

chemistry
given the equilibrium constant for the following reaction at 500 K, 2 NO (g) + O2 (g) <==> 2 NO2 (g) Kc = 6.2x10^5 calculate the equilibrium constant for the reaction expressed as partial pressures, Kp. the answer is 1.51x10^4. How do i get this?
Wednesday, March 28, 2012 at 5:00pm by alex

Chemistry
Please help, I am having trouble solving these problems at nonstandard temperatures. Methanol burns in oxygen to form carbon dioxide and water. Using the balanced reaction, 2CH3OH(l) + 3OH2(g) --> 2CO2(g) + 4H2O(g) 1) Calculate delta H(rxn) in kJ at 24 degrees Celsius 2...
Sunday, July 18, 2010 at 7:30pm by Miguel

chemistry
For the reaction below, Kp= 28.63 at 800 K. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PpCl5=0.5600 atm and PpCl3= 0.4700 atm PCl5(g) <--> PCl3(g) + Cl2(g) PCl5=?? PCl3=?? Cl2=??
Monday, November 5, 2012 at 6:06pm by brun

Chemistry
At 319K the decomposition of dinitrogen tetroxide occurs with the following Kp: 2NO2(g)<>2NO(g)+O2(g) Kp=.700 What is the value of Kc for this reaction?
Sunday, November 27, 2011 at 4:14pm by Tina

Chem11
The reaction 2 COF2(g)--> CO2(g) + CF4(g) has Kp = 2,001,051 at a certain temperature. What would be the value of Kp for the related reaction: 3 CO2(g) + 3 CF4(g)--> 6 COF2(g)? (Enter your answer in scientific notation, e.g. 5.46e-17.)
Monday, May 2, 2011 at 11:46pm by Ryan

Chemistry Help PLEASE!!
I don't know how to do this question, I understand we have to use ICE but I keep getting the wrong answer when I solve for x, it's just not working for me. Consider the following reaction: A(g) -> 2B (g) Find the equilibrium partial pressures of A and B for each...
Friday, February 24, 2012 at 10:15pm by Student

Chemistry
I think you are missing the boat. Kp for 2NO + O2 ==> 2NO2 Kp = 1.48E3 You want Kp for 2NO2 ==> 2NO which is just the reverse of the original equation. For that the new Kp = 1/old Kp (i.e., just the reciprocal of old Kp).
Tuesday, March 9, 2010 at 5:06pm by DrBob222

chemistry
Calculate the value of the equilibrium constant (Kp) for the reaction shown, if F(g) was found to be 96.80 % decomposed at 1000 K when its initial pressure was 4.638 atm. The initial pressure of the reaction products is 0 atm. 2F(g) = F2(g)
Thursday, April 8, 2010 at 9:28pm by andy

CHEMISTRY
Kp = 4 = partial pressure of A x partial pressure of B 4=p*p 4 = p^2 p=2 atm partial pressure A = 2 atm at eqilibrium. partial pressure of B = 2 atm at equilibrium. Kp = Kc(RT)delta n You know Kp and you know R and T. You can calculate delta n (it's mols reactants - moles ...
Sunday, March 18, 2012 at 5:05pm by DrBob222

Chemistry/Equilibrium calculations
I noticed I rewrote the Kp as 1x10^-22 instead of 1x10^-13. Sorry. In the comparison of Kp with Qp for the reverse reaction we have: Kp=10^13 > Qp=10^5, leading to the conclusion that CO is still changing to CO2 as it escapes and its concentration decreases as I ...
Saturday, August 16, 2008 at 7:59am by GK

chemistry
Tricky, tricky. You will notice that the two Kc values given are for different reactions. What you must do is to multiply equation 2 by 4, reverse it, and add it to equation 1. The result is the equation they want for Kp; i.e., P4(s) + 6Cl2 ==> PCl3(l) So if you do that...
Wednesday, July 20, 2011 at 3:25pm by DrBob222

Chemistry
For 1/2 the reaction, new k is sqrt Kp. For 2 x reaction, new k is K^2p For the reverse and 1/2 new k is 1/sqrt Kp.
Monday, February 20, 2012 at 9:10pm by DrBob222

chemistry help!!!!!
Consider the following reaction: Find the equilibrium partial pressures of A and B for each of the following different values of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm, and that the initial partial pressure of A is 0.0 atm. Make any ...
Sunday, March 11, 2012 at 9:57pm by student

chemistry
If you want Kp is it Kp = (PCl5)/(PCl3)(Cl2) Substitute and solve for Kp. I assume Keq is Kc although I don't know that. You can convert Kp to Kc by Kp = Kc(RT)delta n</sup) where delta n = #n products- #n reactants = 1-2 = -1
Wednesday, October 19, 2011 at 3:23pm by DrBob222

chemistry
It's easier than it looks on the surface. Let's call Kp = 3.5 x 10^4 the original Kp. The second equation is just 1/2 of the first one; therefore, new Kp = (original Kp)1/2. If you had 2N2 + 6H2 <==> 4NH3, then new Kp = (original Kp)2 . In other words, ...
Thursday, November 29, 2007 at 5:30pm by DrBob222

chemistry
How do you figure out the answer for the reverse reaction? At 350 K the value of Kp for the equilibrium represented by the balanced equation is 2.87 x 10-2. Calculate the value of Kc for the reverse reaction at the same temperature. Express answer in scientific notation. 2NOBr...
Tuesday, April 13, 2010 at 11:19pm by andy

Chemistry
In which direction will the net reaction proceed X(g)+Y(g)<---->Z(g) Kp=1.00 at 300k for each of these sets of initial conditions? a) [X]=[Y]=[Z]=1.0 m net reaction goes to the left net reaction goes to the right reaction is at equilibrium I chose 3 for a. b) Px=...
Tuesday, February 5, 2013 at 10:57pm by Anon

chemistry
If the initial pressure of H2S(g) is 7.404 atm, calculate the % decomposition of H2S(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 1132 °C is 0.0265. The initial pressure of the reaction products is 0 atm.
Wednesday, October 6, 2010 at 12:52am by Anonymous

Chemistry
Kp=1.78 at 250 degrees for the decomposition reaction, PCl5(g)->PCl3(g)+Cl2(g. Calculate the percentage of reactant that remains if 10.0 moles of starting material are placed in a closed vessel at this temperature and 2.00 atm pressure. Also, determine the value of Kc ...
Wednesday, March 24, 2010 at 9:03am by Jamie

Chemistry
Find delta G knot for the following reaction: 2Ch3OH(l) + 3O2(g) --> 2CO2(g) + 4H2O(g)
Monday, January 2, 2012 at 4:20pm by Summer

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

Chem 1046
Consider the reaction: I2(g) + Cl2(g) 2 ICl(g) Kp = 81.9 at 25°C Calculate ΔGrxn for the reaction at 25°C under each of the following conditions: (a) standard conditions (b) at equilibrium (c) PICl = 2.48 atm; PI2 = 0.321 atm; PCl2 = 0.219 atm
Monday, July 9, 2012 at 2:15pm by Anonymous

Chemistry
A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial pressures: P(SO2)=0.35 atm, P(SO2Cl2)=0.19 atm, P(Cl2)=0.24 atm. Kp=91 for the equilibrium system: SO2 (g) + Cl2 (g) -> SO2Cl2 (g) Is the system at ...
Sunday, February 18, 2007 at 10:43am by Hannah

Chemistry
Kp = pNH3*pH2S Substitute partial pressures and solve for Kp. Then convert Kp to kc by Kp = Kc*RTdelta n
Tuesday, February 19, 2013 at 1:34pm by DrBob222

chemistry
In the fifth reaction of Glycolosis, G3P dehydrogenase converts glyceraldehydes-3-phosphate into glycerate-1,3-bisphosphate. In order to make the reaction spontaneous at biological conditions it must be coupled to the reduction of NAD+. a) DG° for the reaction of just G-3-...
Wednesday, February 11, 2009 at 8:18pm by kat

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
If the initial pressure of NH3(g) is 0.7317 atm, calculate the % of NH3(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 500.0 °C is 67100.00. The initial pressure of the reaction products is 0 atm. 2NH3(g) = N2(g)+...
Sunday, October 3, 2010 at 9:14pm by Kyo

chemistry
What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) --><-- 4 PCL3(l) Given the following at 200 C P4(s)+ 10 Cl2(g) --><-- 4 PCl5(s) Kc=8.12 PCl3(l)+ Cl2(g) --><-- PCl5(s) Kc=0.771 Answer: 6...
Wednesday, July 20, 2011 at 3:25pm by l

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 ...
Saturday, August 16, 2008 at 7:59am by GK

chemistry
Kp for the reaction CO2(g) + C(s) 2CO(g) is 1.47 at 727°C. 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
Calculate the equilibrium constant for 2CH3OH(l)+3O2(g)->2CO2(g)+4H2O(l)
Tuesday, May 17, 2011 at 11:02pm by sara

chemistry
For reactions in solution, molar concentrations are usually used in equilibrium constant expressions (designated by K or Kc). In gases, partial pressures can also be used (designated by Kp). Equilibrium partial pressures of NOCl, NO and Cl2 in a container at 300 K are 1.2 atm...
Wednesday, April 10, 2013 at 9:31am by alex

college chemistry
please help! If the initial pressure of I2(g) is 1.738 atm, calculate the % decomposition of I2(g) when the reaction comes to equilibrium according to the balanced equation. The value of Kp at 1000 K is 0.254. The initial pressure of the reaction products is 0 atm. I2(g) = 2I(g)
Tuesday, October 5, 2010 at 2:41pm by sparkle

chemistry
Consider the following reaction: I2(g) + Cl2(g) 2ICl(g) o Kp = 81.9 at 25 C. Calculate ∆Grxn for the reaction at 25 C under each of the following conditions: a Standard conditions. b At equilibrium. c PICl = 2.55 atm; PI2 = 0.325 atm; PCl2 = 0.221 atm.
Thursday, April 18, 2013 at 10:59am by Melanie

chemistry
If the initial pressure of NH3(g) is 7.845 atm, calculate the % of NH3(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 600.0 °C is 455000.00. The initial pressure of the reaction products is 0 atm. 2NH3(g) = N2(g)+...
Monday, April 12, 2010 at 1:38am by bme1

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
The reaction in the question is the reverse of the reaction given. That is just 1/Kp or 1/11000 = ??
Thursday, September 24, 2009 at 1:35pm by DrBob222

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

chemistry
I also had a problem with this type of questionthe initial pressure of NOCl(g) is 4.329 atm, calculate the % of NOCl(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 400.0 °C is 1.99. The initial pressure of the ...
Thursday, April 8, 2010 at 12:23am by andy

Ap Chem
Why is it possible for Kp to be less than Kc? If this is the case then when Kc>1 it favors products, but if Kp <1 than how can that reaction favor products? Or does that rule only apply for Kc
Sunday, October 9, 2011 at 10:47am by Jane

Chemistry
Consider the hypothetical reaction below. If the initial pressure of A was 2.58 atm, what would be the partial pressure of C (in atm) at equilibrium? KP = 13.6 at 298 K 2 A <==> B + C
Sunday, June 13, 2010 at 1:09pm by Pratana

Chemistry
Hydrogen and methanol (CH3OH) have both been proposed as alternatives to hydrocarbon fuels. a) Write balanced chemical equations for the complete combustion of hydrogen and the complete combustion of gaseous methanol. Combustion reaction for hydrogen: 2H2(g)+ O2 --> ...
Thursday, November 4, 2010 at 1:30am by Jarrod

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

science
Given the following reaction, with Kp=1.05 at 250 degrees C what is Kc? The reaction is PCl5 to PCl3+Cl2
Tuesday, April 13, 2010 at 1:54pm by Nick

chem
How many CO2 molecules would be formed from the reaction mixture that produces the greatest amount of products? 2CH3OH(g)+3O2(g)--->2CO2(g)+4H2O(g)
Wednesday, October 1, 2008 at 3:12pm by natash

Kinetics Problem II
The data below were collected for the following reaction: 2NO2 (g) + F2 (g) ->2NO2F(g) A: Calculate the value of the rate constant, k. B: What is the overall order of the reaction?
Wednesday, January 30, 2013 at 12:51am by Amy

chemistry
If the initial pressure of SO3(g) is 4.775 atm, calculate the % of SO3(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 1000 K is 24.40. The initial pressure of the reaction products is 0 atm. 2SO3(g) = 2SO2(g)+O2(g) ...
Wednesday, April 7, 2010 at 12:23am by bme1

chemistry
The value of delata h for the reaction below is -186 kJ. Calculate the heat Kj released from the reaction of 25g of Cl2
Friday, January 27, 2012 at 4:05am by ashely

chemistry
Calculate the equilibrium constant for 2CH3OH(l)+3O2(g)->2CO2(g)+4H2O(l) by using standard reduction potentials?
Wednesday, May 18, 2011 at 1:33am by KAyla

Chemistry-w/addition
1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs? moles = grams/molar mass. Solve for moles. M = moles/L. Solve for M. 2. What is the pressure in atmospheres of SbCl5 in the container before any decomposition occurs? Use...
Saturday, January 15, 2011 at 2:13pm by DrBob222

Chem II
I'm not exactly sure of what you want but I can give you a start, perhaps. This is a redox reaction. The beginning concns are too high on the right; therefore, the reaction must shift to the left to reach equilibrium. [You can show this by Qp = 0.115/0.215 = 0.534 and this...
Tuesday, October 2, 2012 at 10:02pm by DrBob222

CHEMISTRY HELP!
Consider the following reactions and their equilibrium constants. (NO(g) + 0.5Br2(g) <===> NOBr(g) Kp = 5.3 2NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030 Use these equations and their equilibrium constants to determine the equilibrium constant for the ...
Wednesday, April 27, 2011 at 11:51pm by jon

chemistry -drbob222 (correction)
work for 2: (typo, correction below) Kp = [(1.0-x)/ 10]/[x/ (100)] =2.7 Kp = [(1/28-x)/ 10]/[x/ (100)] =2.7 Kp = [([1/28]^2-x)/ 10]/[x/ (100)] =2.7 x=(1/28)^3 g
Friday, October 9, 2009 at 5:48am by Anonymous

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