For the Equilibrium H 2 O(g)+ CH 4 (g)$\leftrightarrows$ CO(g)+ 3 H 2 (g),K p = 1$\times$

The Answer of For the Equilibrium H 2 O(g)+ CH 4 (g)$\leftrightarrows$ CO(g)+ 3 H 2 (g),K p = 1$\times$

For the Equilibrium H 2 O(g)+ CH 4 (g)$\leftrightarrows$ CO(g)+ 3 H 2 (g),K p = 1$\times$

The Answer of For the Equilibrium H 2 O(g)+ CH 4 (g)$\leftrightarrows$ CO(g)+ 3 H 2 (g),K p = 1$\times$

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For the Equilibrium H₂O(g)+ CH₄(g) $\leftrightarrows$ CO(g)+ 3 H₂(g),K_p = 1 $\times$

question 81

Multiple Choice

For the equilibrium H₂O(g) + CH₄(g) $\leftrightarrows$ CO(g) + 3 H₂(g) ,K_p = 1.61 $\times$ 10^-5 at 1400 K.At a given point,the partial pressures of the gases are $For the equilibrium H2O(g) + CH4(g) \leftrightarrows CO(g) + 3 H2(g) ,Kp = 1.61 \times 10-5 at 1400 K.At a given point,the partial pressures of the gases are = 0.264 atm, = 0.126 atm, = 0.0382 atm,and = 0.0974 atm.Which of the following statements is true? A) Q < K so the reaction will continue to make more products. B) Q > K so the reaction will consume products to make more reactants. C) Q = K so the system is at equilibrium. D) The value of K will decrease until it is equal to Q. E) The value of K will increase until it is equal to Q.$ = 0.264 atm, $For the equilibrium H2O(g) + CH4(g) \leftrightarrows CO(g) + 3 H2(g) ,Kp = 1.61 \times 10-5 at 1400 K.At a given point,the partial pressures of the gases are = 0.264 atm, = 0.126 atm, = 0.0382 atm,and = 0.0974 atm.Which of the following statements is true? A) Q < K so the reaction will continue to make more products. B) Q > K so the reaction will consume products to make more reactants. C) Q = K so the system is at equilibrium. D) The value of K will decrease until it is equal to Q. E) The value of K will increase until it is equal to Q.$ = 0.126 atm, $For the equilibrium H2O(g) + CH4(g) \leftrightarrows CO(g) + 3 H2(g) ,Kp = 1.61 \times 10-5 at 1400 K.At a given point,the partial pressures of the gases are = 0.264 atm, = 0.126 atm, = 0.0382 atm,and = 0.0974 atm.Which of the following statements is true? A) Q < K so the reaction will continue to make more products. B) Q > K so the reaction will consume products to make more reactants. C) Q = K so the system is at equilibrium. D) The value of K will decrease until it is equal to Q. E) The value of K will increase until it is equal to Q.$ = 0.0382 atm,and $For the equilibrium H2O(g) + CH4(g) \leftrightarrows CO(g) + 3 H2(g) ,Kp = 1.61 \times 10-5 at 1400 K.At a given point,the partial pressures of the gases are = 0.264 atm, = 0.126 atm, = 0.0382 atm,and = 0.0974 atm.Which of the following statements is true? A) Q < K so the reaction will continue to make more products. B) Q > K so the reaction will consume products to make more reactants. C) Q = K so the system is at equilibrium. D) The value of K will decrease until it is equal to Q. E) The value of K will increase until it is equal to Q.$ = 0.0974 atm.Which of the following statements is true?

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For the Equilibrium H2O(g)+ CH4(g) ⇆\leftrightarrows⇆ CO(g)+ 3 H2(g),Kp = 1 ×\times×

Definitions:

For the Equilibrium H₂O(g)+ CH₄(g) $\leftrightarrows$ CO(g)+ 3 H₂(g),K_p = 1 $\times$