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| 1 . |
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A chemical system is at equilibrium Online Text [Hint]
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| 2 . |
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What is the relationship between the rate constants for the forward and reverse reactions and the equilibrium constant for a process? Online Text [Hint]
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| 3 . |
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Both the forward and reverse reactions of the following equilibrium are believed to be elementary steps: CO(g) + Cl2(g)  COCl(g) + Cl(g) At 25°C the rate constants for the forward and reverse reactions are 1.4 x 10-28 M-1 s-1 and 9.3 x 1010 M-1 s-1, respectively. What is the value for the equilibrium constant at 25°C? Online Text [Hint]
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| 4 . |
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Suppose that the reactions A --> B and B --> A are both elementary processes with rate constants of 9.6 x 102 s-1 and 3.8 x 104 s-1, respectively. (a) What is the value of the equilibrium constant for the equilibrium A B? (b) Which is greater at equilibrium, the concentration of A or the concentration of B? Online Text [Hint]
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| 5 . |
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Write the expression for Keq for the following reaction: N2(g) + O2(g) 2NO(g) Online Text [Hint]
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| 6 . |
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What is the expression for Keq for the reaction 2N2O(g) + O2(g) 4NO(g)? Online Text [Hint]
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| 7 . |
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For the gas-phase reaction CO + 3H2 CH4 + H2O, which expression represents Keq correctly? Online Text [Hint]
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| 8 . |
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Write the expression for Keq for the following reaction: 2C2H4(g) + 2H2O(g) 2C2H6(g) + O2(g) Online Text [Hint]
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| 9 . |
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What is the expression for Keq for the reaction N2(g) + 3H2(g) 2NH3(g)? Online Text [Hint]
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| 10 . |
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In which of the following reactions is Keq independent of the pressure? Online Text [Hint]
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| 11 . |
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The equilibrium constant for the reaction 2NO(g) N2(g) + O2(g) is Keq = 2.4 x 103 at 2000°C. Calculate Keq for N2(g) + O2(g) 2NO(g). At this temperature does the equilibrium favor NO or does it favor N2 and O2? Online Text [Hint]
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| 12 . |
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Given the equilibrium constant, Keq, of 2.40 x 10-3 at 1000 K for N2(g) + 3H2(g) 2NH3(g), what is the equilibrium constant for NH3(g) 1/2N2(g) + 3/2H2(g) at 1000 K? Online Text [Hint]
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