Chemical Equilibrium & Chemical Kinetics

The rate law for the reaction is rate = k[A] [B] . The order of reaction is

• Zero

• 2/3

• 1/3

• 5/3

The half-life of following first order reaction A → B + C is 10min. The

concentration of A would be reduced to 12.5% of original concentration in

• 30 min

• 40 min

• 70 min

• 90 min

In the given reaction 2A + B →products , it is observed on quadrupling the conc.

of B, rate of reaction increases 16times. The order of reaction with respect to B is

• 0

• 1

• 2

• -1

If rate constant for any reaction is equal to rate of reaction at all concentrations. Then the order of reaction will be

• Zero

• One

• Two

• Three

The rate of chemical reaction roughly doubles for every 10

oC rise of temperature. If temperature is raised by 20 C, the rate may become

• 4 times

• 16 times

• 8 times

• 8 times

In Rate = k[A][B] the second order reaction become ____ if [A] is in large excess

• 2nd order

• 3rd order

• Zero order

• Pseudo 1st order

Determine partial pressure of NO at equilibrium if partial pressure of N2 and O2 are 2 and 8 torr respectively (Kp = 4.0) N2 + O2 2NO

• 8 torr

• 16 torr

• 4 torr

• 64 torr

For the reaction A + B C + D one starts with 6 moles A and 7 moles B per dm3. When equilibrium is attained, 4.5 moles of C is formed, what is the value of Kc for the reaction

• 3

• 1.8

• 3.78

• 5.4

Kc value for decomposition of HF is 10–13 at 2000°C it means that

• Reactants are more stable

• Products are more stable

• Reactants are unstable

• Reactants and products are equally stable

At equilibrium, relationship between concentrations of reactants and products

• [Reactants] > [Products]

• [Reactants] = [Products]

• [Reactants] < [Products]

• All are possible