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a.) A 2.0 L-reaction flask initially contains 0.04 mol CO, 0.23 molH2, and 0.60 mol CH3OH (methanol). If this mixture is brought incontact with a zinc oxide-chromium(III) oxide catalyst, theequilibrium shown below is attained.
CO(g) + 2 H2(g) <---> CH3OH(g)
The equilibrium constant Kc for this reaction at 300°C is 1.110-2.
What is Q?

b.)Hydrogen bromide dissociates when heated according to thefollowing equation.
2 HBr(g) <---> H2(g) + Br2(g)
The equilibrium constant Kc equals 1.6 10-2 at 200°C. What are themoles of substances in the equilibrium mixture at 200°C if we startwith 0.021 mol HBr in a 1.3-L vessel?
HBr(g)__ mol
H2(g)___mol

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Irving Heathcote
Irving HeathcoteLv2
18 Mar 2019

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Related questions

1. The value of Keq for the following reaction is 5.0 x 10-9
BaCO3(s) <--> Ba+2(aq) + CO32-(aq)

What statement is most correct about the equilibrium reactionmixture?
products dominate
reactants dominate
There is a reasonable mixture of reactants and products
only products exist.
only reactants exist.

2.For the reaction FeO(s) + CO(g) Fe(s) + CO2(g),
-the usual expression for the equilibrium constant is[Fe][CO2]/[FeO][CO]
-addition of CO2(g) will increase Kc.
-increasing the volume of an equilibrium mixture at constanttemperature will cause the number of moles of CO2 to increase asthe mixture re-equilibrates.
-adding more FeO to an equilibrium mixture will cause the number ofmoles of CO2 to increase as the system re-equilibrates.
-None of the above statements is true

3. Kc for the reaction F2(g) + Cl2(g)<--> 2 FCl(g) equals 125at a particular temperature. Suppose a system involving thisreaction is already at equilibrium and the concentrations of F2 andCl2 are found to be [F2] = 0.115 M and [Cl2] = 0.221 M. What is theconcentration of FCl in the system?
[FCl] = 1.78 M
[FCl] = 3.17 M
[FCl] = 2.54 x 10-2 M
[FCl] = 1.43 x 10-2 M
None of the above is within 5% of the correct answer

4. At high temperatures one mole of hydrogen gas reacts with onemole of bromine gas to form hydrogen bromide. At a giventemperature the equilibrium constant is 57.6. If at the sametemperature, a mixture of 4.67 x 10-3 M hydrogen gas, 2.14 x 10-3bromine gas, and 2.40 x 10-2 M hydrogen bromide gas is made,then
-the system is far from equilibrium and will shift to form morehydrogen gas.
-the system is far from equilibrium and will shift to form morehydrogen bromide gas.
-nothing can be deduced since we do not know whether the reactionis endothermic or exothermic.
-nothing can be deduced since we do not know whether theequilibrium constant is Kc or Kp.
-the system is at equilibrium.

5. Which one of the following equilibriums is least affected by achange in the volume of the system?
2 C(s) + O2(g) <--> 2 CO(g)
H2(g) + S(l) <---> H2S(g)
2 NO2(g)<--->N2O4(g)
H2O(l)<--->H2O(g)
2 NO(g) + Cl2(g)<-->2 NOCl(g)

1. The value of Keq for the following reaction is 5.0 x 10-9
BaCO3(s) <--> Ba+2(aq) + CO32-(aq)

What statement is most correct about the equilibrium reactionmixture?
products dominate
reactants dominate
There is a reasonable mixture of reactants and products
only products exist.
only reactants exist.

2.For the reaction FeO(s) + CO(g) Fe(s) + CO2(g),
-the usual expression for the equilibrium constant is[Fe][CO2]/[FeO][CO]
-addition of CO2(g) will increase Kc.
-increasing the volume of an equilibrium mixture at constanttemperature will cause the number of moles of CO2 to increase asthe mixture re-equilibrates.
-adding more FeO to an equilibrium mixture will cause the number ofmoles of CO2 to increase as the system re-equilibrates.
-None of the above statements is true

3. Kc for the reaction F2(g) + Cl2(g)<--> 2 FCl(g) equals 125at a particular temperature. Suppose a system involving thisreaction is already at equilibrium and the concentrations of F2 andCl2 are found to be [F2] = 0.115 M and [Cl2] = 0.221 M. What is theconcentration of FCl in the system?
[FCl] = 1.78 M
[FCl] = 3.17 M
[FCl] = 2.54 x 10-2 M
[FCl] = 1.43 x 10-2 M
None of the above is within 5% of the correct answer

4. At high temperatures one mole of hydrogen gas reacts with onemole of bromine gas to form hydrogen bromide. At a giventemperature the equilibrium constant is 57.6. If at the sametemperature, a mixture of 4.67 x 10-3 M hydrogen gas, 2.14 x 10-3bromine gas, and 2.40 x 10-2 M hydrogen bromide gas is made,then
-the system is far from equilibrium and will shift to form morehydrogen gas.
-the system is far from equilibrium and will shift to form morehydrogen bromide gas.
-nothing can be deduced since we do not know whether the reactionis endothermic or exothermic.
-nothing can be deduced since we do not know whether theequilibrium constant is Kc or Kp.
-the system is at equilibrium.

5. Which one of the following equilibriums is least affected by achange in the volume of the system?
2 C(s) + O2(g) <--> 2 CO(g)
H2(g) + S(l) <---> H2S(g)
2 NO2(g)<--->N2O4(g)
H2O(l)<--->H2O(g)
2 NO(g) + Cl2(g)<-->2 NOCl(g)

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