Answer:
a) Q>K because K decreased
b) shift left
Explanation:
According to Van't Hoff equation
d (ln K)/ dT = ΔH/RT²
since ΔH< 0 (exothermic reaction) , then d (ln K)/ dT < 0 → K decreases with an increase in temperature
thus
a) Since Q represents the product of concentrations , and assuming an increase in temperature do not affect significantly the concentration of products in a liquid state , then Q remains approximately constant , but K decreases → Q>K because K decreased
( thus ΔG is positive and ΔG is negative for the reverse reaction → products will produce reactants until the new equilibrium is reached)
b) Since K decreased , the system will shift towards the reactants and thus it will shift to the left
