Consider the following reaction (assume an ideal gas mixture): 2NOBr(g) 2NO(g) + Br2(g) A 1.0-liter vessel was initially filled with pure NOBr, at a pressure of 4.0 atm, at 300 K.
After equilibrium was reached, the volume was increased to 2.0 liters, while the temperature was kept at 300 K. The result of this change was:
a.
an increase in Kp.
b.
a decrease in Kp.
*c.
a shift in the equilibrium position to the right.
d.
a shift in the equilibrium position to the left.
e.
None of these are correct.
At 25°C the reaction is first order in CH3CH2Cl, and the rate constant is 4.3 × 10–3 s–1. If the Ea = 100.0 kJ/mol, what will the rate constant be at 40°C? (R = 8.314 J/mol.K)