If the temperature is lowered what is fa vored 1

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If the temperature is lowered, what is fa- vored? 1. reactants 2. products correct Explanation: 007 3.6points Which of the following will change the value of the equilibrium constant for a reaction? I) changing the concentration of one of the products; II) changing the concentration of one of the reactants; III) changing the temperature. 1. I, II and III 2. III only correct 3. II and III only 4. I only 5. II only 6. I and II only Explanation: Only changing the temperature will change the value of the equilibrium constant. 008 3.6points Consider the reaction Ni(CO) 4 (g) Ni(s) + 4 CO(g) . If the initial concentration of Ni(CO) 4 (g) is 1.0 M, and x is the equilibrium concentra- tion of CO(g), what is the correct equilibrium relation? 1. K c = x 4 1 . 0 - x 4 correct 2. K c = x 4 1 . 0 - 4 x 3. K c = 4 x 1 . 0 - 4 x 4. K c = x 5 1 . 0 - x 4 5. K c = x 1 . 0 - x 4 Explanation: 009 3.6points
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casey (rmc2555) – Homework 5 – holcombe – (51395) 3 Given the reversible reaction equation 2 CO(g) + O 2 (g) 2 CO 2 (g) which is the relationship between K c and K p ? 1. K p = K c ( RT ) 2 2. K p = K c 3. K p = K c RT 4. K p = K c ( RT ) 2 5. K p = K c ( RT ) 1 correct Explanation: The ideal gas law can be used to derive the link between K c and K p : P = n V RT = MRT M = P RT K c = [CO 2 ] 2 [CO] 2 [O 2 ] = P 2 CO 2 ( RT ) 2 P 2 CO ( RT ) 2 · P O 2 RT = P 2 CO 2 P 2 CO · P O 2 RT = K p RT K p = K c ( RT ) 1 010 3.6points Given the following equilibria and equilibrium constants K 1 CO(g) + H 2 O(g) CO 2 (g) + H 2 (g) K 2 CH 4 (g) + H 2 O(g) CO(g) + 3 H 2 (g) K 3 CH 4 (g) + 2 H 2 O(g) CO 2 (g) + 4 H 2 (g) The correct expression for K 3 in terms of K 1 and K 2 is 1. K 3 = K 1 + K 2 2. K 3 = K 1 K 2 3. Cannot be determined from this informa- tion. 4. K 3 = K 1 K 2 correct 5. K 3 = K 1 - K 2 Explanation: CO(g) + H 2 O(g) CO 2 (g) + H 2 (g) K 1 = [CO 2 ][H 2 ] [CO][H 2 O] CH 4 (g) + H 2 O(g) CO(g) + 3 H 2 (g) K 2 = [CO][H 2 ] 3 [CH 4 ][H 2 O] Adding (1) and (2), CO(g) + H 2 O(g) + CH 4 (g) + H 2 O(g) CO 2 (g) + H 2 (g) + CO(g) + 3 H 2 (g) CH 4 (g) + 2 H 2 O(g) CO 2 (g) + 4 H 2 (g) K 3 = [CO 2 ][H 2 ] 4 [CH 4 ][H 2 O] 2 K 1 K 2 = parenleftbigg [CO 2 ][H 2 ] [CO][H 2 O] parenrightbigg parenleftbigg [CO][H 2 ] 3 [CH 4 ][H 2 O] parenrightbigg = [CO 2 ][H 2 ] 4 [CH 4 ][H 2 O] 2 = K 3 011 3.6points Consider the reaction NH 4 (NH 2 CO 2 )(s) 2 NH 3 (g) + CO 2 (g) . What is the relationship between K and K c ? 1. K = ( RT ) 2 K c 2. K = ( RT ) 3 K c correct 3. K c = ( RT ) 2 K 4. K = RT K c 5. K c = ( RT ) 3 K
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casey (rmc2555) – Homework 5 – holcombe – (51395) 4 Explanation: 012 3.6points The balanced equation for a particular reac- tion has 4 moles of gaseous reactants and 2 moles of gaseous products. For this reaction at room temperature, which of the following would be true? 1. K c is unrelated to K p 2. K c equals K p 3. K c is less than K p 4. K c is greater than K p correct Explanation: n gas products = 2 n gas reactants = 4 K c and K p are related by the equation K p = K c ( RT ) Δ n where Δ n = n gas products - n gas reactants = 2 - 4 = - 2 Since Δ n is a negative number, the value of K p will be smaller than the value of K c ; this can also be stated as K c being greater than K p .
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