Chemistry: Principles and Practice
3rd Edition
ISBN: 9780534420123
Author: Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: Cengage Learning
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Chapter 17, Problem 17.91QE
(a)
Interpretation Introduction
Interpretation:
The value of equilibrium constant for the reaction at
(b)
Interpretation Introduction
Interpretation:
The value of equilibrium constant for the reaction at
(c)
Interpretation Introduction
Interpretation:
The value of equilibrium constant for the reaction at
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X,(g) X(g)
Assume that the standard molar Gibbs energy of formation of X(g) is 4.43 kJ - mol' at 2000. K and -53.56 kJ · mol- at 3000.
K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature.
At 2000. K, AG = 4.43 kJ · mol. What is K at that temperature?
K at 2000. K =
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The equilibrium constant for the reaction, 3 H2(g) + N2(g)= 2NH3(g), at a given temperature is 1.4 x 10–7. Calculate the equilibrium concentration of ammonia, if [H2] = 1.2 x 10–2 mol L–1 and [N2] = 3.2 x 10–3 mol L–1.
Nitrogen and oxygen react at high temperatures.(a) Write the expression for the equilibrium constant (Kc) for the reversible reactionN2(g) + O2(g) ⇌ 2NO(g) ΔH = 181 kJ
Chapter 17 Solutions
Chemistry: Principles and Practice
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