A first order reaction takes 100 minutes for completion of 60% of the reaction.  Find the time when 90% of the reaction will be completed.

In general it is observed that the rate of chemical reaction doubles with every 10^o rise in temperature.  If the generalization holds good for the reaction in the temperature range 295 K to 305 K, what would be the value of activation energy for the this reaction?
(R = 8.314 J mol^-1  K^-1)

The reaction,
N₂(g) + O₂(g) \(\rightleftharpoons \)2NO(g)
Contributes to air pollution whenever a fuel is burnt in air at a high temperature.  At 1500 K, equilibrium constant K for it is 1.0 \(\times\) 10^-5.  Suppose in a case [N₂] = 0.80 mol L^-1and [O₂] = 0.20 mol L^-1 before any reaction occurs. Calculate the equilibrium concentration of the reactants and the product after the mixture has been heated to 1500 K.

The half-life for the decomposition of nitramide is 2.1 hour at 15 ^oC
NH₂NO₂(aq) \(\to\) N₂O (g) + H₂O(l)
If 6.2 g of NH₂NO₂ is allowed to decompose, calcualte
(i) time taken for NH₂NO₂ to decompose 99%
(ii) volume of N₂O (dry) produced at STP.

The half-life for the reaction:
N₂O₅ \(\to\) 2NO₂ + \(1\over2\)O₂ is 2.4 hours at 30 ^oC.
(a) Starting with 100 grams of N₂O_s, how many gram will remain after 9.6 hours?
(b) What time would be required to reduce 5 \(\times\) 10¹⁰ molecules of N₂O₅ to 10⁸ molecules?

The reaction between A and B is first order with respect to A and zero order with respect to B.  Fill in the blanks in the following table:

The rate constants of a reaction at 500 K and 700 K are 0.02 s^-1 and 0.07 s^-1 respectively.  Calculate the values of E_a and A.

The gas phase decomposition of CH₃OCH₃ follows first order kinetics
CH₃OCH₃ ⟶ CH₄(g) + H₂(g) + CO(g)
The reaction is carried out in a constant volume container at 500⁰ C and has t_1/2 = 14.5 min. Initially only dimethyl ether is present at a pressure of 0.40 atm. What is the total pressure of the system after 12 min? Assume ideal behavior.