The reduction of NO by H2 has been studied for decades. If a flask contains 0.65 M nitrogen monoxide, 0.28 M water vapor, 0.31 M nitrogen gas, and 0.225 M hydrogen gas, compare the reaction quotient Qc to Kc and predict whether the reaction will shift towards products or reactants. 2 NO(g)+2H2(g) *) 2 H2O(g)+N2(g) Kc = 0.022
(a) (10 pts) Q value:
(b) (5 pts) ○ It is impossible to make this prediction ○ Reaction is at equilibrium ○ Reaction will shift towards products ○ Reaction will shift towards reactants ○ None of the above
The reduction of NO by H2 has been studied for decades. If a flask contains 0.65...
I said that the answer was D because I got 83.3333 as the answer which would make Qc>Kc sending the equation to the right towards the products. Please explain why I am right or wrong and please provide the correct answer with an explanation if I am incorrect. Thank you Consider the following reaction and its equilibrium constant: 12(g) + Br2(g) = 2 IBr(g) Kc = 1.1 x 102 A reaction mixture contains 0.49 M 12, 0.30 M Br2 and...
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5 pts Question 4 A mixture of 0.75 moles of H2S. 0.40 moles of H2, and 1.25 moles of S2 are placed in a 10.0L container. Which of the following statements is true if the following reaction has a Ke value of c.40 x 108 at a temperature of 750°C? 2 H25 (8)2H2(g) + S2 (8) The reaction shifts to the right to establish equilibrium The reaction is already at equilibrium The value of K will change as the reaction...
The general form of a chemical reaction is aA + bB = cC +dD Where A and B are reactants in the forward direction and C and D are products in the forward direction. The lower case letters are the stoichiometric coefficients for the balanced equation. The general form of the equilibrium constant equation is then: Keq = [C]c[D]d/[A]a[B]b Part I: Q vs. K Q: reaction quotient can be calculated for a reaction at any concentration values of reactants and...