18) as reaction is reversed.
Kc = (1/Kc)1/2
=> (1/1.08×107)1/2
=> 9.62×10-4
19) increasing the concentration of N2
Question 18 Given the following equation and equilibrium constant, 2 H2 (9) + S2(9)=2 H2S(g) Kc...
Given the following equation and equilibrium constant, 2 H2(g) + S2(o)=2 H2S(g) Kc -1.08 x 107 Determine Ke for the following reaction H2S(g) + H2(g) + 2.70 X 106 1.35 * 106 3.01 x 10-4 2.31 x 10-8 Moving to another question will save this response
> Click Submit to complete this assessment. Question 22 Given the following equation and equilibrium constant, 2 H2(g) + S2(o)=2 H2S(g) Ke=1.08 x 107 Determine Ke for the following reaction. H25(9) =Hz()+ 526) 2.70 x 106 1.35 X 106 3.04 x 10-4 2.31 x 10-8
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QUESTION 2 Consider the following reversible reaction at equilibrium: 3H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the products (right side)? Decreasing the amount of NH3. Increasing the temperature. Adding a catalyst to the system. Decreasing the amount of H2. Increasing the volume of the system.
8. Consider the reaction: 2 H2S(g) 2 H2(g) +S2(g) Kc = 1.67 x 107 at 800°C What is the value of Kp at this temperature?
For the equilibrium H2(g) + S(s) ⇔ H2S(g), Kc = 6.1 x 105 at 298 K. If the concentrations of H2 and H2S are equal, which of the following statements is true? A. The reaction quotient is 1. B. The concentrations of H2 and H2S can never be equal. C. The concentration of S equals Kc. D. The equilibrium constant equals 1. E. The system is at equilibrium.
QUESTION 1 11 poin Given the following endothermic reaction, predict which way the reaction will shift to re-establish equilibrium after being disturbed by each action below 2A) + 3 Bad Cam + 2DG) Removing some C A Toward the reactant side Adding more B. The reaction will not shift in response to the action - Adding more C. The reaction will shift, but there is not enough information to determine which way it was shift - Removing Toward the product...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced? decreasing the volume adding N2 increasing the volume adding H2 2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced? decreasing the temperature adding H2 increasing the temperature adding N2 3. What is the effect of a...
#9,10,11 9. Given the reaction below: 2502 H2(g) + S(s) <--> 2 H2S (9) a. Write Kc, the equilibrium expression, for the reactions above. 10. Find Kc, the equilibrium expression, for the reactions above. The concentrations are 2.75 M H2, .78 MS, and 0.24 M H2S. 11. Based on the calculation for Kc above, is this reaction a product favored or a reactant favored equilibrium?
Consider the following system at equilibrium. N2(g) + 3 H2 (g) 2 NH3(g) + 92.24 kJ <--> Which response includes all of the following that will shift the equilibriu to the right, and no others? I. increasing the temperature III. increasing the pressure II. decreasing the temperature IV. decreasing the pressure VI. adding some NH3 V. removing some NH3 VII. removing some N2 VIII. adding some N2 a) I, IV, VI, and VII c) I, VI, and VII e) II,...