Consider the equilibrium CH4(g) + H2O(g) <--> CO(g) + 3H2(g), where delta h= 206 KJ. Which...

Consider the equilibrium CH4(g) + H2O(g) <--> CO(g) + 3H2(g), where delta h= 206 KJ. Which of the following disturbances will NOT cause the system to shift to the right to reestablish equilibrium?
A.) The partial pressure of CH4 increases.
B.) The partial pressure of CO decreases.
C.) The volume decreases.
D.) The temperature increases.
E.) All of these will cause the system to shift to the right.

Solutions

Expert Solution

Given equilibrium reaction is CH4(g) + H2O(g) <--> CO(g) + 3H2(g) :delta H= 206 KJ.

According to the Le-Charterlier's principle,

(1) If the temperature is raised, reaction will proceed in the direction in which some heat can destroy (absorbed) so that temperature of the system remains constant.

Thus increase in temperature shifts the equilibrium in the forward direction of those reactions which proceed with absorption of heat (endothermic reactions), and in the back ward direction of those reactions which proceed with the evolution of heat (exothermic reactions)

(2) If the pressure is increased, reaction will takes place in a direction which will bring about lowering f pressure. This implies that the equilibrium will shifts in the direction which produces the smaller no. of gas molecules.

(3) If the concentration of reactants is increased or product is removed , the reaction will take place in the forward direction. If the concentration of reactants decreases or increasing the concentration of products the reaction will take place in the backward direction.

(4) Catalyst speeds up both forward & backward reactions to the same extent but does not have any effect on Equilibrium point.

(5)---> When the no. of moles of reactants & products are same the addition of inert gas has no effect

----> for a reaction at constant pressure ,addition of an inert gas will shifts the equilibrium in the direction in

which there is increase in the no . of moles of the gases

A.) The partial pressure of CH4 increases.---> reaction proceeds in forward direction(towards right)
B.) The partial pressure of CO decreases.----> reaction proceeds in forward direction(towards right)
C.) The volume decreases.-----> reaction proceeds in forward direction(towards right)
D.) The temperature increases. ------> reaction proceeds in forward direction(towards right)
So All of these will cause the system to shift to the right.

Therefore option (E) is correct

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

Part A: For the reaction CO(g) + 3H2(g) ---> CH4(g) + H2O(g) (delta)H° = -206.1 kJ...

Part A: For the reaction CO(g) + 3H2(g) ---> CH4(g) + H2O(g) (delta)H° = -206.1 kJ and (delta)S° = -214.7 J/K The standard free energy change for the reaction of 1.54 moles of CO(g) at 293 K, 1 atm would be (?) kJ. This reaction is (reactant, product)(?) favored under standard conditions at 293 K. Assume that (delta)H° and (delta)S° are independent of temperature. Part B: For the reaction I2(g) + Cl2(g) --> 2 ICl(g) (delta)G° = -30.0 kJ and...

For the following equilibrium reaction: CO + 3H2 <---> CH4 +H2O + HEAT a) Describe what...

For the following equilibrium reaction: CO + 3H2 <---> CH4 +H2O + HEAT a) Describe what will happen to the concentration of CO when you cool this reaction? b) Describe what will happen to the CH4 concentration when you add hydrogen gas to the reaction? c) Draw the energy diagram for this reaction. Be sure to show the relative total energy of the reactants and of the products. Also, identify the activation energy for this reaction on your energy diagram.

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g),...

For the equilibrium system CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), ΔH = -206 kJ/mol, state whether the yield of CH4 will increase, decrease or remain the same for the following changes: Adding some H2 gas to the system Removing H2O from the system Increasing the volume of the system Decreasing the temperature on the system Adding a catalyst to the system

consider the following system at equilibrium where delta H = 16.1 kj, and Kc = 6.50x10^-3,...

consider the following system at equilibrium where delta H = 16.1 kj, and Kc = 6.50x10^-3, at 298 K. 2NOBr forwsrd reverse arrows 2NO + Br2 if the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Kc: increases decreases remains thesame the value of Qc: is greater than Kc equal to Kc is less than Kc the reaction must: run in the forward direction to restablish equilibrium run in the reverse remain the same....

Consider the following system at equilibrium where Kc = 0.159 and delta H° = -111 kJ/mol...

Consider the following system at equilibrium where Kc = 0.159 and delta H° = -111 kJ/mol at 723 K. N2(g) + 3 H2(g) = 2 NH3(g) The production of NH3(g) is favored by: Indicate True (T) or False (F) for each of the following: ___TF 1. increasing the temperature. ___TF 2. decreasing the pressure (by changing the volume). ___TF 3. increasing the volume. ___TF 4. adding NH3. ___TF 5. removing H2.

Consider the following system at equilibrium where Delta H° = 108 kJ, and Kc = 1.29×10-2,...

Consider the following system at equilibrium where Delta H° = 108 kJ, and Kc = 1.29×10-2, at 600 K. COCl2(g) <---> CO(g) + Cl2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value of Kc A. increases. B. decreases. C. remains the same. The value of Qc A. is greater than Kc. B. is equal to Kc. C. is less than Kc. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run...

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23...

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23 at 25 °C. 1.50 mol CH4 and 2.50 mol H2O are added to an empty 2.00-L container at 25 °C and allowed to reach equilibrium. What are the equilibrium amounts (in moles) of each species? The answer is: 1.5 mol CO, 4.5 mol H2 , 1.0 mol H2O, and 2.6×10–21 mol CH4. Please include written work and explanation :-) Thank you!

Consider the reaction CO(g) + 3 H2 (g) ⇌ CH4 (g) + H2O(g) Kc = 7.7×10–23...

For C(s) + H2O(g) ⇌ CO(g) + H2(g) H = +. In which direction will the...

For C(s) + H2O(g) ⇌ CO(g) + H2(g) H = +. In which direction will the reaction shift if heat is removed from the system, C is added, H2O is removed, CO is added, and H2 is removed. (a) right, left, no change, left, right (b) left, left, right, left, right (c) left, right, left, left, right (d) left, no change, left, left, right (e) None of the above

If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g)

If delta H rxn is -75.2 kJ, 2NO(g) + Cl2 (g) <---> 2NOCl(g) A scientist places four moles of nitrogen monoxide and two moles of chlorine gas into flask A and the same amounts into Flask B, then allows the systems to reach equilibrium. Flask A is at 25 degrees Celsius and Flask B is at 200 degrees Celsius A) In which flask will the reaction occur faster? Explain. B) In which flask will the reaction occur to a greater...

Subjects