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
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?
Question 7 (5 points) Consider the equilibrium below: CO(g) + H2O(g) = CO2(g) + H2(g) Kc = 0.0611 at 2000 K If Pco and PH20 are both initially 2.95 atm, what will be the equilibrium partial pressure of H2? Express your answer in decimal format to 3 significant figures. Your Answer: N. Answer Coal, which is primarily carbon, can be converted to natural gas (primarily methane, CH4) by the following exothermic reaction: + C(s) 2H2(g) CH4(g) Which of the following...
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.
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...
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.
#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?
2 H2S(g) ⇌ 2 H2(g) + S2(g) Kc = 9.0 × 10−8 at 700°C the initial concentrations of the three gases are 0.500 M H2S, 0.500 M H2, and 0.250 M S2. Determine the equilibrium concentrations of the gases.
2. How is the equilibrium-constant expression (Kc) for the reaction: 2NO(a) = N2() + Ke=0.145; related to the following reaction? O2 (a) N2(a) + O2(a) = 2NO(a) K=.............. (b) 4NOQ = 2Nz () + 2O2(g) Kos......... (c) NO) 1/2 N2(0)+ 1/2O2(0) K3= +++ (d) 1/2 N2(a) + 1/2O2(a) = NO) Ke=.............. 3. Given Kc or ko for the following reactions, what is the value of Koor K? (a) l2(g) + Cl2(a) = 2ICIOX Kc = 2.0 x105 at 25°C (b)...