Chemistry Question Bank

In Fe(CO)5, the Fe – C bond possesses

Consider the following complex ions, P, Q and R. P = [FeF6]3- , Q = [V(H2O)6]2+ and R = [Fe(H2O)6]2+ The correct order of the complex ions, according to their spin-only magnetic moment values (in BM) is

The rate of formation of NO2 during the period 600 – 700 s is

The instantaneous rate of reaction at the beginning of the reaction is

Assertion (A): If the activation energy of a reaction is zero, temperature will have no effect on the rate constant. Reason (R): Lower the activation energy, faster is the reaction.

Assertion (A): The order of a reaction can have fractional value. Reason (R): The order of a reaction cannot be written from balanced equation of a reaction.

Assertion (A): In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients. Reason (R): It is the mechanism and not the ba…

Choose the correct answer out of the following choices. Assertion (A): Most people think diamond is forever. Reason (R): Conversion rate of diamond to graphite is very low.

Collision theory is used to explain how chemical species undergo a reaction. Using this theory and the kinetic molecular model, which of the following does NOT influence the rate of a chemical reaction?

For a first order reaction A P, the temperature (T) dependent rate constant (k) was found to follow the equation 1 logk 6.0 T . The pre- exponential factor A and the activation energy Ea, respectively are: (a) 1.0…

An endothermic reaction with high activation energy for the forward reaction is given by the diagram : (a) (b) (c) E E (d)

The potential energy diagram for a reaction R P -> is given below o H of the reaction corresponds to the energy:

Ea and H values of reactions R1, R2, R3 and R4 carried out at the same temperature are as given below: R1 Ea = 40 kJ mol–1, H = – 80 kJ mol–1 R2 Ea = 20 kJ mol–1, H = – 30 kJ mol–1 R3 Ea = 60 kJ mol–1, H = + 40 kJ mol…

The first order rate constant for a certain reaction increases from 1.667 × 10–6 s–1 at 727ºC to1.667 × 10–4 s–1 at 1571ºC. The rate constant at 1150ºC, assuming constancy of activation energy over the given temperatu…

In most cases, for a rise of 10K temperature the rate constant is doubled to tripled. This is due to the reason that (a)collision frequency increases by a factor of 2 to 3. (b)fraction of molecules possessing threshol…

For a certain reaction A -> products, the t1/2 as a function of [A]0 is given as below: [A]0 (M) : 0.1 0.025 t1/2 (min) : 100 Which of the following is/are true ?

The reaction of hydrogen and iodine monochloride is given as: H g 2ICl g 2HCl g I g -> The reaction is of first order with respect to H2 (g) and ICl(g), following mechanisms were proposed. Mechanism A: H g 2…

The hypothetical reaction A B 2AB; -> follows the following mechanism Fast A A A, -> Slow Fast A B AB B,A B AB. -> -> The order of the overall reaction is

The initial rates of reaction 3A + 2B + C -> Products, at different initial concentrations are given below: Initial rate M s–1 [A]0 , M [B]0 , M [C]0 , M 5.0 × 10–3 0.010 0.005 0.010 5.0 × 10–3 0.010 0.005 0.015 1.0 ×…

For the reaction : sunlight H Cl 2HCl ->

From the following data find rate constant of decomposition of H2O2 in aqueous solution Time (in minutes) Volume (in cc of KMnO4) 22.8 13.3 8.25

1 mL of ethyl acetate was added to a flask containing 20 mL of N/20 HCl maintained at 25oC. 2 mL of the reaction mixture were withdrawn at different intervals and titrated with a standard alkali solution. The followin…

The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume. 2(g) 2(g) 2(g) SO Cl SO Cl -> Experimen t Time/s-1 Total pressure/atm 0.5 0.6 What is the rate of reaction…

Hydrolysis of methyl acetate in aqueous solution has been studied by titrating the liberated acetic acid against sodium hydroxide. The concentration of the ester at different times is given below. t/min C/mol L-1 0.85…

Half-lives of a first order and a zero order reaction are same. Then the ratio of the initial rates of first order reaction to that of the zero order reaction is (a) 0.693