Question

Predict the effect of the following changes on the reaction H2 (G) + CO2 (g) <--->...

Predict the effect of the following changes on the reaction

H2 (G) + CO2 (g) <---> H2O (g) +CO (g) . Delta H= 90.0 kcal

(a) Adding CO2

(b) Adding H20

(c) Increasing the temp.

(d) Decreasing the volume of the container

Homework Answers

Answer #1

a)
we are adding a reactant
According to Le Chatelier's Principle,
Adding reactant will shift reaction towards product side
Answer: Equilibrium moves to product side

b)
we are adding a product
According to Le Chatelier's Principle,
Adding product will shift reaction towards reactant side
Answer: Equilibrium moves to reactant side

c)
Forward reaction is endothermic in nature
we are increasing temperature or adding heat here
so, according to Le Chatelier's principle,
equilibrium will move in direction which absorbs heat
hence, forward reaction will be favoured
Answer: Equilibrium moves to product side

d)
We are decreasing volume here
In other words we are trying to increase pressure
so, according to Le Chatelier's principle,
Reaction will try to decrease the pressure
Hence it will move in a direction which have lesser gaseous molecules

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift...
Determine how each of the following changes will affect the equilibrium reaction below (shift left, shift right, no change) H2O(g) + C(s) ↔ H2(g) + CO(g) ∆H° = 131 kJ a. increasing the temperature b. adding CO c. removing H2 c. removing H e. increasing the volume of the container f. adding more carbon to the reaction
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the...
Consider the following reaction. CO (g) +H2O (g) = CO2 (g) + H2 (g) If the reaction begins in a 10.00 L vessel with 2.5 mol CO and 2.5 mol H2O gas at 588K (Kc= 31.4 at 588 K). Calculate the concentration of CO, H2O, CO2, and H2 at equilibrium.
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M...
Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=102 at 500 K A reaction mixture initially contains 0.120 M COand 0.120 M H2O. A)What will be the equilibrium concentration of [CO]? B)What will be the equilibrium concentration of [H2O]? C)What will be the equilibrium concentration of [CO2]? D)What will be the equilibrium concentration of [H2]?
The gas phase equilibrium reaction is exothermic : 4NH3(g)+5O2(g) <----->4NO(g)+6H2O(g) What is the effect of each...
The gas phase equilibrium reaction is exothermic : 4NH3(g)+5O2(g) <----->4NO(g)+6H2O(g) What is the effect of each of the following? A) Decreasing the volume B) increasing/adding H2O C) increasing the temperature D) removing some oxygen E) increasing/adding NH3 F) adding a catalyst
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g)...
CO2 and H2 are allowed to react until equilibrium is established as follows: CO2(g) + H2(g) ↔ H2O(g) + CO(g) Which of the following changes will cause the equilibrium position to shift to the right? a. increase in the concentration of H2 b. decrease in the concentration of CO c. decrease in the concentration of CO2 d. more than one correct response e. no correct response
for the reaction 47kcal+2SO3(g)-2SO2(g)+O(g) predict the effect on the position of equilibrium will it shift to...
for the reaction 47kcal+2SO3(g)-2SO2(g)+O(g) predict the effect on the position of equilibrium will it shift to the left or to the right or will there be no change for each of the following changes the temperature is increased the pressure is increased by decreasing the volume of the container
28) Consider the following reaction at equilibrium in a closed container: Zn(s) + 2HCl(aq) ⇌ Zn2+(aq)...
28) Consider the following reaction at equilibrium in a closed container: Zn(s) + 2HCl(aq) ⇌ Zn2+(aq) + 2Cl-(aq) + H2(g) Which of the following changes WILL NOT affect the equilibrium of the system? A) increasing the concentration of HCl(aq) B) adding Zn to the solution C) decreasing the pressure of H2 D) adding ZnCl2 to the solution E) decreasing the volume of the container
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for...
Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g) A) Find Kp for this reaction at 298 K B) What is 1) Consider the water-gas shift reaction: H2(g) + CO2(g) = H2O(g) + CO(g). A) Find Kp for this reaction at 298 K. B) What is ΔH° for this reaction? C) What type of pressure and temperature change would favor CO production? D) What is K at 1000 K?
The water gas shift reaction is used commercially to produce H2(g): CO(g)+H2O(g)⇌CO2(g)+H2(g). Use the following data...
The water gas shift reaction is used commercially to produce H2(g): CO(g)+H2O(g)⇌CO2(g)+H2(g). Use the following data to determine: ΔfH∘[CO2(g)] = -393.5 kJ/mol ΔfH∘[H2(g)] = 0 kJ/mol ΔfH∘[CO(g)] = -110.5 kJ/mol ΔfH∘[H2O(g)] = -241.8 kJ/mol ΔS∘[CO2(g)] = -393.5 Jmol−1K−1 ΔS∘[H2(g)] = -393.5 Jmol−1K−1 ΔS∘[CO(g)] = -393.5 Jmol−1K−1 ΔS∘[H2O(g)] = -393.5 Jmol−1K−1 a. ΔrH∘ at 298 K. b. ΔrS∘ at 298 K. c. ΔrG∘ at 298 K. d. K at 650 K .
Assume that the following endothermic chemical reaction is at equilibrium: C(s) + H2O(g) ⇔ H2(g) +...
Assume that the following endothermic chemical reaction is at equilibrium: C(s) + H2O(g) ⇔ H2(g) + CO(g) All of the following will increase the ratio of products to reactants in the equilibrium mixture EXCEPT Group of answer choices removal of a gaseous prduct. decreasing the pressure. increasing the volume. increasing the temperature. addition of solid carbon.