For the reaction: A(g) +2 B(g) 2 C(g) +2 D(g) the equilibrium constant is 0.575 at 25.0 °C and 0.775 at 50.0 °C. Making the approximation that AH and AS do not change with the temperature, calculate the values of AH, AS, and the equilibrium constant, K, at 100.0 °C. What would be the value of Q (the heat) if this reaction took place at constant volume? Calculate the value of W (the work) for this reaction at a constant pressure of 1.00 atm at 25.0°C.

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Chapter1: Chemical Foundations
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For the reaction:
A(g) +2 B(g) 2 C(g) +2 D(g)
the equilibrium constant is 0.575 at 25.0 °C and 0.775 at 50.0 °C. Making the
approximation that AH and AS do not change with the temperature, calculate the
values of AH, AS, and the equilibrium constant, K, at 100.0 °C. What would be the
value of Q (the heat) if this reaction took place at constant volume? Calculate the value
of W (the work) for this reaction at a constant pressure of 1.00 atm at 25.0°C.
Transcribed Image Text:For the reaction: A(g) +2 B(g) 2 C(g) +2 D(g) the equilibrium constant is 0.575 at 25.0 °C and 0.775 at 50.0 °C. Making the approximation that AH and AS do not change with the temperature, calculate the values of AH, AS, and the equilibrium constant, K, at 100.0 °C. What would be the value of Q (the heat) if this reaction took place at constant volume? Calculate the value of W (the work) for this reaction at a constant pressure of 1.00 atm at 25.0°C.
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