Number of results: 8,730
The following reaction has an equilibrium constant of 0.020 at a given temperature. 2HI(g) I2(g) + H2(g) If you have 1.00 mol HI(g) in a 0.750-L container initially, how many moles of HI(g) will be present when the system reaches equilibrium?
Thursday, November 18, 2010 at 5:40pm by Adrianne
2NO(g) + H2(g) --> N2O(g) + H2O(g) + energy. 1. Assume the reaction is reversible and at equilibrium. What shifts in the equilibrium of this reaction are suggested by Le Chateliers Principle?
Monday, March 26, 2012 at 2:22pm by John
For the reaction mc011-1.jpg at 472°C equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37 x 10-8M. What is the equilibrium constant for this reaction
Monday, November 25, 2013 at 3:04am by mike
chemistry check my work
the equilibrium-constant expression for a reaction is kc= [N2][H2O]2 ---------- [NO]2[H2] what is the equilibrium-constant expression when the equation for this reaction is halved and then reversed? 2NO + 2H2 --> N2 + 2H2O NO + H2 ---> N + H2O N + H2O --> NO + H [NO][...
Wednesday, April 14, 2010 at 10:02pm by Anna
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.400 M. N2 (g) + O2 (g) --> 2NO (g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established?
Sunday, February 17, 2013 at 2:49pm by Jefferson
Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3. (A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius. (B) What will be the new equilibrium concentrations if the volume of the ...
Thursday, April 22, 2010 at 10:33pm by Frank
H2(g) + I2(g) 2 HI(g) The forward reaction above is exothermic. At equilibrium, what happens if I2 is removed from the reaction mixture at constant temperature and volume? The reaction absorbs energy. The reaction releases energy. [H2] increases. [H2] decreases. [H2] remains ...
Sunday, September 19, 2010 at 9:32pm by Megan
N2 (g) + H2 (g) <--> NH3 (g) + energy Name the direction of equilibrium shift - The pressure of the system is increased. - H2 is added to the system. - The temperature of the system is decreased.
Sunday, April 8, 2012 at 11:54pm by Anonymous
I am having a hard time with this problem. I was wondering where I went wrong. The problem says The equilibrium constant, Kc, for the reaction of H2 and N2 is 1.7×10^2 at 225 ∘C. 3H2(g)+N2(g)←→2NH3(g) If the system at equilibrium contains 0.16M H2 and 0.026M ...
Wednesday, November 13, 2013 at 9:56pm by chelsea
What is the predominant intermolecular force responsible for the dissolution of the hydrophilic end of soap in water? Using dashed lines, illustrate where the intermolecular force occurs between atoms in adjacent molecules? Lone pair electrons have been omitted in the ...
Sunday, June 30, 2013 at 6:10pm by Angela
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
For the following reaction, the equilibrium constant Kc = 97.0 at 900K. If the initial concentrations of NH3 and H2S are both 0.20 M, what is the equilibrium concentration of H2S? H2S(g) + NH3(g) = NH4HS(s) Would you have to create an ICE chart for this type of problem?
Saturday, March 17, 2012 at 7:30pm by David
Consider the following equilibrium process at 686 C C02(g)+H2(g)=CO(g)+H20(g) The equilibrium concentration of the reacting species are [CO]=0.050M, [H2]=0.045M, [CO2]=0.086M, and [H20]=0.040M. (a)Calculate the Kc for the reaction at 686 C. (b) If we add CO2 to increase its ...
Sunday, April 25, 2010 at 1:04pm by Amphee
Start with an equation H2 + I2 -> 2HI so 2 moles of HI formed for each mole of I2 used. at start 0.100 M/L (H2) and 0.100 M/L (I2) at equilibrium 0.0213 M/L (I2) so 0.0787 M/L I2 used so 0.1574 M/L HI formed and 0.0213 M/L equlibrium concentration of H2 Kc=[HI]^2/[H2][I2] ...
Friday, September 30, 2011 at 8:33am by Dr Russ
Consider the following reaction at equilibrium: C(s) + H2O(g) CO(g) + H2(g) Predict which of these stresses which cause the equilibrium system to shift towards the reactant side (to the left). (There may be more than one correct answer - choose ALL of the correct choices.) a. ...
Monday, May 2, 2011 at 11:54pm by Ryan
The question below, i was wondering if it decrease because the N2 is on the right and so to add to left it would be too much so it gets rid of it by decreases and doing to the right? because the left side is (+) endothermic? sorry im a little confused. if the number was ...
Monday, October 25, 2010 at 11:03pm by Ben
If Kc = 0.143 at 25°C for this reaction, find the equilibrium concentrations of C6H12 and CH3C5H9 if the initial concentrations are 0.200 M and 0.075 M, respectively. a. [C6H12] = 0.041 M, [CH3C5H9] = 0.041 M b. [C6H12] = 0.159 M, [CH3C5H9] = 0.116 M c. [C6H12] = 0.241 M, [...
Sunday, January 30, 2011 at 4:28pm by bob
In an equilibrium mixture of HCl, Cl2 and H2, the partial pressure of H2 is 4.2 mPa and that of Cl2 is 8.3 mPa. What is the partial pressure of HCl at 500 oK given that at that temperature Kp = 4.0 x 1018 for H2(g)+ Cl2(g)--> 2HCl(g)
Tuesday, May 31, 2011 at 10:53pm by jj
Kc = 1.87 10-3 for the following reaction. PH3BCl3(s)=>PH3(g) + BCl3(g) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.400...
Saturday, February 7, 2009 at 12:13am by Ashley
CHEM desperate help!
What is the Kc for the following equilibrium CO2(g)+H2(g)←→CO(g)+H2O(g) if [CO] = 0.32M , [H2O] = 0.26M , [CO2] = 0.30M , and [H2] = 3.3×10−2M ?
Sunday, July 28, 2013 at 10:31pm by Anonymous
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. Ans.: ...
Sunday, October 9, 2011 at 10:47am by Jane
After 4.00 mol of C2H4(g) and 2.50 mol of Br2 (g) are placed in a sealed 1.0L container, the reaction reaches equilibrium and is written following: C2H4(g) + Br2(g) -> C2H4Br2(g) ... Calculate the equilibrium concentrations of all three substances.
Thursday, August 9, 2012 at 3:17pm by Sarah
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.500 M. The balanced chemical equation is N2+O2<--->2NO. If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after ...
Tuesday, April 2, 2013 at 3:02pm by Dee
For the system 2SO2(g) + O2(g) <--> 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L container. The system is allowed to reach ...
Saturday, January 12, 2008 at 10:45pm by S
When carbon dioxide is heated in a closed container, it decomposes into carbon monoxide and oxygen according to the following equilibrium equation: 2CO2(g) 2CO(g) + O2(g) When 2.0 mol of CO2(g) is placed in a 5.0-L closed container and heated to a particular temperature, the ...
Monday, March 31, 2008 at 7:26am by Laureta
for the equilibrium H2+CO2<-->H2O+CO Kc=3.18 at 1106K. if each of the four species was initially present at 3.000M calculate the equilibrium concentration of the CO at this temperature..... OK I can get as far as equilibrium (final) H2O=3.000-x CO=3.000-xx H2=3.000+x CO2...
Sunday, May 9, 2010 at 11:14pm by Andy
Chloroacetic acid has a relatively large equilibrium constant, so at low acid concentrations it is necessary to use the quadratic equation in order to calculate the concentrations of the aqueous species. Ka for ClCH2COOH is 1.4 ´ 10-3. For the problems that follow, consider ...
Saturday, June 19, 2010 at 3:43am by leona
C(s) + H2O(g) ⇌ CO(g) + H2 ΔH>0 For the system above at equilibrium, which changes will increase the amount of H2(g)? I. Adding C(s) II. Increasing the volume of the container III. Increasing the temperature The answer is II and III. I understand everything ...
Friday, March 29, 2013 at 12:57am by Ash
Correct the equation to N2 + 3H2 ==> 2NH3 Set up an ICE chart. initial: N2 = 1 mole/2 L = 0.5 M H2 = 3 moles/2 L = 1.5 M NH3 = 0 change: NH3 = +2x N2 = -x H2 = -3x equilibrium: N2 = 0.5-x H2 = 1.5-3x NH3 = 2x Substitute into Kc expression and solve. Post your work if you ...
Wednesday, April 14, 2010 at 5:23pm by DrBob222
For the equilibrium system: H2 + F2 <----> 2HF Kc = 230 If 5.80 mol of hydrogen gas and 5.80 mole are added to a 1.00 L flask what will be the concentration of HF at equilibrium?
Thursday, April 15, 2010 at 6:00pm by Sue
can the concentrations of reactant and products affect the directions of equilibrium constant
Friday, April 23, 2010 at 2:26am by bme1
The equlibrium constant Kc for the reaction: has the value of 4.00 at 500K. If a mixture of 1.00 mol CO and 1.00 mol H2O is allowed to reach equilibrium at this temperature in a 1.00L flask, calculate the equilibrium concentrations of each species in the flask.
Sunday, April 11, 2010 at 6:11pm by curtis
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
Please show step by step with answer The equilibrium constant for the reaction C (s) + H2O (g) <---> CO(g) + H2 (g) is 0.20 at 1000 degrees Celsius. If an equilibruim mixture contains solid carbon, H20 = 0.40 M, and CO = 0.41 M, what is the H2?
Monday, May 31, 2010 at 4:43pm by Lynne
Can someone explain how to do this problem? For the equilibrium reation below, 288g of liquid water and 448 g of carbon monoxide are placed in an 8.00 liter container and heated to 900 K. If the value of K_c for the reaction at 900 K is 1.56, what are the equilibrium ...
Tuesday, May 25, 2010 at 1:25pm by Anonymous
Consider the following reaction. CaSO4(s) Ca2+(aq) + SO42-(aq) At 25°C the equilibrium constant is Kc = 2.4 10-5 for this reaction. (a) If excess CaSO4(s) is mixed with water at 25°C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca2+ and ...
Saturday, October 20, 2012 at 2:02pm by Olivia
I completed a lab to find the determination of Kc. I have to find the concentrations of reactants at equilibrium using an ICE table. The equation that were are using is Fe^3+(aq) + SCN^-(aq) -> Fe(SCN)^2+(aq) I have to create 5 ICE tables because we used 5 different test ...
Monday, March 5, 2012 at 1:51pm by Hannah
9 mol HI(g)is sealed with H2(g)in an empty 2 dm container when equilibriup is reached by the reaction..H2(g)+I2(g)=2HI(g) at 130 C it found that there are 5 mol HI(g)in the equilibrium mixture.calculate the equilibriup constant
Thursday, January 31, 2013 at 10:53am by Lillian nhlapo
The equilibrium constant, Kc is 3.2 x10 -34 at 25C for the reaction 2 HCl(g) <=> H2(g) + Cl2(g). what is The equilibrium expression, Kc for the reaction
Wednesday, April 27, 2011 at 5:26pm by Donna
An equilibrium was established after 0.100 mol of hydrogen gas and 0.100mol of iodine gas were added to an empty 1.00L reaction vessel and heated to 700K. The color intensity of the mixture changed from deep purple to a lighter purple color. At equilibrium, concentration of ...
Friday, September 30, 2011 at 8:33am by Dominique
If the equilibrium concentrations are [PCl5] = 1.0M, [Cl2] = 0.10M, what is the equilibrium constant value? PCl5(g) <---> PCl3(g) + Cl2(g) Would you mind showing the calculations Please. I've been working on this problem over an hour now. Not certain if I am working it ...
Sunday, January 20, 2013 at 3:40pm by Cathy
Chemistry Equilibrium Constant
The initial pressures for I2 (g), H2(g), and HI(g) were Pi2 = 0.100 atm, Ph2 = 0.200 atm, and Phi = 0 atm, respectively. After the system came to equilibrium, the pressure of I2 (g) became very low, PI2 = 1.00 x 10^-5 atm. Calculate the equilibrium constant Kp for this reaction
Sunday, March 18, 2012 at 11:15pm by Raskin
A 0.25 mol sample of n204 dissociates and comes to equilibrium in a 1.5 L flask at 100 degrees C. The reaction is N2O4 > 2 NO2. The Kc at 100 degrees C is 0.36. What are the equilibrium concentrations of NO2 and N2O4?
Saturday, July 20, 2013 at 5:21pm by Marie Genvieve
A quantity of electrical charge that brings about the deposition of 4.5 g Al from Al3+ at a cathode will also produce what volume (STP) of H2(g) from H+ at a cathode? I know there are 3 e- difference b/w the two reactions. I took 4.5 g/3 and get 1.5 g H2. Then (1.5 g H2)(1 mol...
Sunday, October 9, 2011 at 12:34am by Holly
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
Given the equilibrium: CO + 2H2 = CH3OH H=-18.0kJ How will the concentration of CO at equilibrium be affected by the following? a) Adding more CH3OH b) Removing some H2 c) Reducing the temperature. I don't understand how i'm supposed to figure these out.. please help!
Tuesday, May 31, 2011 at 1:38pm by Amber
For the reaction 2NH3(g) 3H2(g) N2(g) at 472oC equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37x10^_8 M. What is the equilibrium constant for the reverse reaction?
Monday, July 16, 2012 at 12:58pm by joe
That's 0.15 WHAT and 0.05 WHAT? You add whatever it is. It is either mols, molar, or atm pressure. I will assume it is M since you say "concentrations." but you can change that as needed. ..........H2 + I2 ==> 2HI I......0.15M...0.05M...0 C........-x.....-x.....2x E......0....
Friday, May 4, 2012 at 5:05pm by DrBob222
The concentrations didnt show up correctly...they should be H2=[.513] Br2=[..62] 2HBr=[.346] thank you!
Monday, January 18, 2010 at 7:55pm by mary
H2+CO2<==>H2O+CO 1. what changes in concentrations of the products can be made to shift the equlilbrium to the right.?
Saturday, May 8, 2010 at 8:47pm by briget
For the reaction H2+I2, Kc=55.3 at 700K. In a 2. L flask containing an equilibrium mixture of three gases, there are .056g H2 and 4.36 g I2. What is the mass of the I2 in the flask?
Monday, January 31, 2011 at 12:11pm by Jeff
The tendency of water/solvent to flow from concentrations where solute concentrations are high across a membrane to concentrations where solute concentrations are low to give an equal water/solvent to solute ratio on both sides of the membrane.
Friday, February 1, 2013 at 1:55am by Devron
For the reaction, 2 SO2(g) + O2(g) == 2 SO3(g), at 450.0 K (Kelvin) the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations, (SO3) = 0.254 M and (O2) = 0.00855 M, and (SO2) = 0.500 M. In which direction will it go? A. to the...
Saturday, March 3, 2012 at 9:52pm by Hannah
You have the equation. Convert 1 mol to molarity. 1 mole/3 liters. Set up an ICE chart, plug in the numbers and solve for the unknown. Subtract from 1/3 to find how much H2 remains after equilibrium is established, then multiply by 3 L to find moles H2.
Tuesday, March 17, 2009 at 10:50pm by DrBob222
I assume the masses measured were before the experiment started; i.e., what you started with. If so, then change each of these to mols/dm^3. The titrations were to find the equilibrium concentrations of the components. Use M x dm^3 = #mols, convert # mols per whatever volume ...
Saturday, November 1, 2008 at 4:28pm by DrBob222
The following equilibrium pressures were observed at a certain temperature for the reaction. N2(g) + 3 H2(g) <==> 2 NH3(g) partial pressure of NH3 = 3.2 ✕ 10−1 atm partial pressure of N2 = 1.6 ✕ 10−2 atm partial pressure ...
Friday, November 8, 2013 at 3:17pm by Anonymous
A substance (CD) decomposes into C and D At the temperature of the experiment, 15.0% of CD is decomposed when equilibrium is established. a) if the initial concentration of CD is 0.200mol/L, what are the equilibrium concentrations of CD, C and D? I got 0.17 for CD and I got 0....
Wednesday, April 4, 2012 at 10:11pm by Danielle
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.570 mol IBr in a 2.50-L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2?
Wednesday, February 20, 2013 at 9:03pm by Hannah
For the reaction I2(g) + Br2(g) 2 IBr(g), Kc = 280. at 150.°C. Suppose that 0.590 mol IBr in a 2.50-L flask is allowed to reach equilibrium at 150.°C. What are the equilibrium concentrations of IBr, I2, and Br2?
Monday, February 6, 2012 at 7:41pm by Stan3000
The following table contains data for the equilibrium reaction CH3COOH(g)+ C2H5OH(g)↔ CH3COOC2H5(g)+ H2O(g) T = 100oC. Each row in the table represents a different experiment (diffferent intial concentrations). Initial concentration Equilibrium concentration...
Thursday, September 24, 2009 at 1:29pm by Ava
the concentrations and pressures at equilibrium were found to be: 1.6 × 10–2 M for A, 8.1 × 103 Pa for B, 13.6 M for C, 13.1 M for D, and 3.9 × 104 Torr for E. Calculate the equilibrium constant, K the right answer is 1x10^12 i tried this problem so many times and i cannot ...
Wednesday, March 13, 2013 at 9:04pm by jane
The reaction CO(g) + H2O(g)--> CO2(g) + H2(g) has Kc = 102 at 500 K. If a reaction mixture initially contains 0.154 M CO and 0.154 M H2O, what will be the equilibrium concentration of H2?
Monday, May 2, 2011 at 11:50pm by Ryan
For H2(g) + Br2(g) -> 2HBr(g) k=64 <- Ice table: H2 Br2 HBr I 0.10 0.10 0 C -x -x +2x E Solve for HBr at equilibrium I do not know how to start this.
Wednesday, February 29, 2012 at 9:01pm by Hannah
please help w/ chem hw
An equilibrium mixture at 225∘C contains 8.0×10−2M NH3 and 0.20M H2 for the reaction 3H2(g)+N2(g)←→2NH3(g) If the Kc at this temperature is 1.7×102, what is the equilibrium concentration of N2?
Sunday, July 28, 2013 at 10:33pm by Anonymous
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(check my work)
The initial concentration for the compounds involved in the reaction shown were determined to be [CS2(g)] = 1.075 mol/L, [H2(g)] = 1.436 mol/L, [CH4(g)] = 0.6740 mol/L, [H2S(g)] = 0.3120 mol/L. Calculate the value of the equilibrium constant (Kc) at 1175 K if the equilibrium ...
Tuesday, April 6, 2010 at 9:01pm by bme1
A 1.00 L flask containing the equilibrium mixture CO +Cl2 <-> COCl2 was found to contain 0.400 mol of COCl2, 0.100 mol of CO, and 0.500 mol of Cl2. If 0.300 mol of CO is added at constant temperature, what will be the new concentrations of each component at equilibrium?(...
Sunday, April 29, 2012 at 1:51pm by Divya
At a certain temperature, the reaction CO(g) + 2H2(g) <===> CH3OH(g) has Kc = 0.500. If a reaction mixture at equilibrium contains 0.00436 M CH3OH and 0.220 M H2, what is the equilibrium concentration of CO? The answer is 0.280 M. I dont know how to get it.
Wednesday, April 27, 2011 at 9:33pm by chris
Which of the following is a true statement about chemical equilibria in general A.there is only one set of equilibrium concentrations that equal teh Kc value B.eqauilibrium is the result of cessation of all chemical change C.at equilibrium the rate of the forward reaction is ...
Tuesday, May 11, 2010 at 7:26pm by Dave
This is a question on Le Chatelier's Principle. Basically that principle tells us that a system in equilibrium will try to undo what we do to it. That isn't what you read in a text but it is one way to look at it. So if we ADD H2 to the system it will try to undo that. How can...
Saturday, October 15, 2011 at 3:19pm by DrBob222
Consider the equilibrium, A + B <--> C, with K=32.217 and initial concentrations of A,B, and C, of 3.665M, 0.883M, and 3.925M, respectively. What is the equilibrium concentration of B 3.665 0.883 3.925 A + B = C Keq=(C)/(A)*(B)= 32.217 Q = (3.025)/(3.665)*(0.883)=1.21 Q...
Wednesday, February 7, 2007 at 5:31pm by Rob
Chemistry - Equilibrium
Silver ion concentrations are needed for a solution. You have 0.050 M AgNO3, if you added 5.0mL of 12. M NH3 to 500.mL of this solution, how much silver ion in M will you have at equilibrium? [Kf for Ag(NH3)2+ is 1.5 x 10^7]
Wednesday, April 25, 2012 at 4:12pm by Shawn
the reaction between H2 and O2 reaches equilibrium in a closed container according to the following balanced equation: 4HCl+O2=2H2O+2Cl2 the volume of the container is 5dm3 calculate the equilibrium constant (Kc) for this reactin
Thursday, March 7, 2013 at 8:53am by tjale
In a study of the following reaction at 1200K it was observed that when the equilibrium partial pressure of water vapor is 15.0 torr, the total pressure at equilibrium is 36.3 torr. 3Fe(s)+4H2O(g) (reversible arrows) Fe3O4(s)+4H2(g) Calculate the value of Kp for this reaction ...
Monday, July 30, 2007 at 5:48pm by Taasha
Are you sure there is no volume given. The following will give you mols at equilibrium. ..........2HI ==> H2 + I2 initial...0.05.....0....0 change....=2x......x.....x equil...0.05-x.....x.....x Kc = 76 = (H2)(I2)/(HI)^2 Solve for x Then x/volume = concn.
Sunday, March 18, 2012 at 7:27pm by DrBob222
the initial concentration of each component was: 0.100 M H2(g), 0.100M I2(g), and 0.050 M HI(g) . The Keq = 50.2. Calculate the concentration of each component when equilibrium has been reached. The balanced chemical equation for this reactions is: H2(g) + I2(g) 2HI(g)
Saturday, April 14, 2012 at 4:36pm by Steve
I answered this question but I did not get the right answer. CO2 + H2 <=> H2O + CO CO2 = 0.5 mole and H2 he 0.5 mole both sollutions were forced into a 1 Litre container. K = 2 what is the equlibrium concentration of each reactant and product. as I calculated I did the ...
Tuesday, May 8, 2007 at 6:31pm by Linda
what are the equilibrium concentrations of Pb2+ and F- in a saturated solution of lead (II)flouride if the Ksp for PbF2 is 3.2*10^-8?
Friday, December 7, 2012 at 8:24pm by Victoria
I'm sure you know the equation for the H2. 2H^+ + 2e ==> H2(g) E=Eo-(0.059/n)*log(pH2/H^+) but you need to add the partial pressures and concentrations to that. Here is a site you can read about the SCE. http://en.wikipedia.org/wiki/Saturated_calomel_electrode
Sunday, November 16, 2008 at 11:04pm by DrBob222
Write the Kc expression, set up an ICE chart, substitute, and solve. moles H2 = 0.763/2.016 and that divided by 3.67 L = M; approximately 0.1 but you need to do it more precisely than that. moles I2 = 96.9g/molar mass I2 and that divided by 3.67 L = about 0.1 M. Again you ...
Sunday, October 17, 2010 at 11:10pm by DrBob222
Add the columns so that initial column + change column = equilibrium column. Equilibrium: CO = 0.145-x H2O = 0.145-x CO2 = x H2 = x Now substitute those values into your Kc expression and solve for x.
Sunday, March 21, 2010 at 8:00pm by DrBob222
The following reaction has an equilibrium constant of 0.50 at a given temperature. HCHO(g) CO(g) + H2(g) If you have 0.55 moles of HCHO(g) in a 1.0L container initially, how many moles of HCHO will be present when the system reaches equilibrium?
Friday, November 19, 2010 at 6:42pm by Adrianne
At equilibrium, the concentrations in this system were found to be [N2] = [O2] = 0.100 M and [NO] = 0.500 M. N2(g) + O2(g) <-> 2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-...
Monday, March 5, 2012 at 10:52pm by David
The equlibrium constant K, for the reaction, H2 + CO2 <-> H20 + CO, is 4.2 at 1650 degrees C. Initially, 0.80 mol H2 and 0.80 mol CO2 are injected into a 5.0L flask. Calculate the concentration of each species at equilibrium.
Sunday, March 18, 2012 at 7:31pm by Kristen
For the equilibrium H2(g)+CO2(g)<-->H2O(g)+CO(g) Kc=3.18 at 1106 K.If each of the four species was initially present at a concentration of 3.000M,Calculate the equilibrium concentration of the CO (g) at this temperature. Choices 0.844 3.268 3.844 3.460 2.156 Thanks ...
Sunday, May 9, 2010 at 10:24pm by Andy
urgent help chemistry!!
2H2 +O2 ---> 2H20 A container at a o degrees celcius is filled with a mixture of oxygen and hydrogen. The fastest way to establish an equilibrium is.. 1. add more H2 2. do nothing, equilibrium will occur 3. increase the temperature 4. increase surface area. which is correct?
Monday, February 14, 2011 at 2:07am by Anonymous
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
Write the Keq expression. Substitute the equilibrium concentrations given. Solve for (O2). Post your work if you get stuck.
Monday, November 10, 2008 at 4:54pm by DrBob222
The equilibrium constant expression is: K(eq)=[N2][O2] / [NO]^2 = 8.36*10^3 Substitute the concentrations given and solve for [NO]
Sunday, January 3, 2010 at 6:47pm by GK
Based on a Kc value of 0.140 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?
Friday, July 12, 2013 at 5:39pm by Anonymous
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.300 mol of H2 and 0.300 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
Saturday, January 19, 2013 at 4:49pm by Paul
the equilibrium constant for the synthesis of HBr(g0 from hydrogen and bromine gas is 2.18*10 exponent 6 at 730 degrees celcius.if 3.75 mol of HBr(g) is put into a 15L reaction vessel,calculate the concentration of H2,Br2 and HBr at equilibrium
Tuesday, April 2, 2013 at 5:53pm by tracy
Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure. The equilibrium constant is 0.12 at 25°C. If you had originally placed 0.036 mol of cyclohexane in a 1.0 L ...
Tuesday, May 24, 2011 at 2:33pm by Kat
The half-cell, Tl | Tl+(1 mol L-1), is connected to a Pt | H+ | H2(1 atm) half-cell in which the concentration of H+ is unknown. The measured cell voltage is 0.0841 V and the Pt | H2 | H+ half-cell is the cathode. Standard reduction potentials are given on the next page. (a) ...
Tuesday, November 27, 2012 at 11:07pm by sabrina
The initial concentration for the compounds involved in the reaction displayed were determined to be [CH4(g)] = 0.9530 mol/L, [H2O(g)] = 0.9911 mol/L, [CO(g)] = 0.7474 mol/L, [H2(g)] = 0.2717 mol/L. Calculate the value of the equilibrium constant (Kc) at 1200 K if the ...
Thursday, September 29, 2011 at 7:21pm by BOB
Le Chatelier's Principle, in not so eloquent terms, says that a reaction at equilibrium will shift to try and undo what we've done to it. a. So if we remove CO2 it will move to the left so as to increase CO2. b. Adding H2 molecules it will shift to the right to try to use up ...
Monday, March 25, 2013 at 7:33pm by DrBob222
the equilibrium composition of a reaction is 1.522mol CO, 1.566mol H2, 0.478mol CH4 and 0.478mol H2O and the volume of the reaction vessel is 10Litres. -What is the equation for the reaction? -Calculate the equilibrium constant for both the forward and reverse reaction?
Tuesday, April 5, 2011 at 4:03am by Taynell
At high temperature, 2.00 mol of CH2O was placed in a 4.00 L container where it decomposed via the equilibrium CH2O(g)<=>CO(g)+H2(g) . At equilibrium, the concentration of CO was measured to be 0.0317 M. What is Kc for this reaction at this temperature?
Saturday, April 20, 2013 at 9:56am by alex
Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 723.0 K: [N2(g)] = 2.936 mol/L, [H2(g)] = 2.933 mol/L, [NH3(g)] = 3.443 mol/L. N2(g)+3H2(g) = 2NH3(g)
Wednesday, October 2, 2013 at 10:22am by plzhelp
At 1285°C, the equilibrium constant for the reaction Br2 (gas) <---> 2Br (gas) is Keq= 1.04 X 10^ -3 A 0.200-L vessel containing an equilibrium mixture of gases has 0.245 g. Br2 (gas) in it. What is the mass of Br (gas) in the vessel? What are the concentrations of Br2 ...
Monday, January 3, 2011 at 5:50am by Mina