I have a few chemical equilibrium and reaction questions I am stuck on.
1) Consider the following chemical equilibrium:
Heat + CO + 2H2 ⇌ CH3OH
Cooling the reaction mixture will...
a. decrease amounts of CO(g)
b. decrease amounts of CH3OH
c. increase amounts of CH3OH
d. decrease amounts of H2
2)
Consider the following chemical equilibrium:
H2 + Cl2 ⇌ 2HCl
Increasing the reaction mixture will...
a. have no effect
b. shift the reaction toward the reactant side
c. shift the reaction toward the product side
d. increase amount of the product
1)
Given equilibrium is
In the given equilibrium, forward reaction is endothermic and backward reaction is exothermic.
According to Lechatlier's principle, when a system is at equilibrium and the factors affecting the equilibrium such as concentration, temperature, pressure... are changed, the equilibrium shifts in a direction to reduce or nullify the the change (OR)
When a stress is applied on a system is at equilibrium, the system moves in a direction to reduce or nullify the stress.
Effect of Concentration : If concentration of reactants is increased, the equilibrium shifts in a direction to reduce the concentration of reactants ie rate of forward reaction increases. Similarly if concentration of products is increased, the equilibrium shifts in a direction to reduce the concentration of products ie rate of backward reaction increases.
Effect of temperature: If forward reaction is exothermic, the backward reaction becomes endothermic. Similarly if forward reaction is endothermic, backward reaction becomes exothermic.
Generally exothermic reactions are favourable at low temperatures and endothermic reactions are favourable at high temperatures.
On cooling, the reaction moves in a direction to increase the temperature. ie exothermic reaction takes place.
Hence backward reaction takes place.
Decreases the amounts of methanol (CH3OH).
Option B is the correct answer.
2)
The given equilibrium is
If the reaction mixture ie Hydrogen and Chlorine gas is increased, the equilibrium shifts in a direction to shift towards right side. ie equilibrium shifts towards products side.
Option C is the correct answer.
Option D is also correct as forward reaction increases, the concentration of products increases.
I have a few chemical equilibrium and reaction questions I am stuck on. 1) Consider the...
1) For the following reaction: SO2Cl2(g)<-> SO2(g) + Cl2 (g) Kp=2.91x10^3 at 298K In the reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of CL2 is 285 torr. The partial pressure of SO2Cl2 is [x]torr. 2) For the following reaction:NH4HS(s)<->NH3(g) + H2S (g) Kc=8.5x10^-3 At any given point the reaction mixture has solid NH4HS, NH3 at 0.166M and H2S at 0.166M. a) Is the reaction at equilibrium? b)Will more of the solid form, or will...
Consider the reaction: CO(g)+2H2(g)⇌CH3OH(g) An equilibrium mixture of this reaction at a certain temperature was found to have [CO]= 0.115 M , [H2]= 0.124 M , and [CH3OH]= 0.235 M . Part A What is the value of the equilibrium constant at this temperature?
27. Consider the following chemical reaction: N2(g) + 2O2(g) ----> 2NO2(g) decreasing the pressure of reaction mixture will decrease amounts of O2(g) have no effect on the reaction increase amounts of N2(g) increase amounts of NO2(g) 26. Consider the following chemical reaction: CO(g) + Cl2(8) ----------> COCl2(g) At the beginning 0.400 M CO(g) is mixed with 0.0500 M C12(8). At equilibrium, 0.0100 M of the product is produced. Calculate the equilibrium constant. K-0.641 K - 1.99x 10exp-3 K-8.81 OK -...
Name: 1. An exothermic reaction is allowed to reach equilibrium. If the temperature of the reaction mixture is decreased, the equilibrium will shift towards the product side: True False [1pt] 2. For the reaction C(s) + H2O(g) CO(g) + H2(g) a decrease in concentration of C(s) will cause the reaction to shift to the left oTrue False [1pt] 3. Define the following terms: [1.5pts] a. Activation Energy b. Exothermic Reaction c. Equilibrium [1p) 4. Determine the equilibrium constant K C(s)...
Consider the reaction CO(g) + 2H2(g) = CH3OH(g) An equilibrium mixture of this reaction at a certain temperature was found to have [CO] = 0.125 M, [H2] = 0.124 M, and (CH3OH) = 0.275 M. Part A What is the value of the equilibrium constant at this temperature? Express the equilibrium constant to three significant figures. IVO AE ? Keq = 181 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
9. Which of the following will have no shift in equilibrium if the volume is decreased? 2H2O(g) + N2(g) + 2H2(g) + 2NO(g) SiO2(g) + 4HF(g) SiF4(g) + 2H2O(g) CO(g) + H2(g) C(g) + H2O(g) C6H1206(s) + 602 6CO2(g) + 6H2O(g) 10. Which of the following will shift this endothermic reaction to the REACTANT side? 302(g) 203(g) Increase the pressure Decrease the O2 gas Increase the temperature Remove the ozone, O3
Consider the following equilibrium: CO(g) + 2H2(g) ⇌ CH3OH(g) + energy Which of the factors below would decrease the concentration of CH3OH at equilibrium? a. a decrease in the temperature b. an increase in the temperature c. an addition of CO d. an increase in H2
Consider the following equilibrium: CO(g) + 2H2(g) ⇌ CH3OH(g) + energy Which of the factors below would decrease the concentration of CH3OH at equilibrium? a. a decrease in the temperature b. an increase in the temperature c. an addition of CO d. an increase in H2
Consider the following equilibrium for which H = 664.38: N2(g) + 2 H2O(g) 2 NO(g) + 2 H2(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction? (a) NO(g) is added to the system. (b) The reaction mixture is heated. (c) The volume of the reaction vessel is reduced by 50%. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding...
oi Prelab 11, Equilibrium Control of a Reaction me Consider the following equilibrium reaction Predict which direction the equilibrium will shift (left, towards reactants or right, towards products) when you perform the following actions: Shift Right Shift Left Action Add CH4 to the reaction Add CO, to the reaction Add CO to the reaction Add H, to the reaction Remove CH4 from the reaction Remove CO2 from the reaction Remove CO from the reaction Remove H2 from the reaction Increase...