If decomposition reaction `A(g) to B(g)` follows first order kinetics then the graph of rate of (R) of B against time t will be :

The gaseous decomposition reaction, A(g) rarr 2B(g) + C(g) is observed to first order over the excess of liquid water at 25^(@) C. It is found that after 10 minutes the total pressure of system is 188 torr and after very long time it is 388 torn The rate constant of the reaction (in hr^(1) ) is: [Given: vapour pressure of H_(2) O at 25^(@) C is 28 torr(In 2 = 0.7, In 3 = 1.1, In 10 = 2.3)]

The reaction mathbf(A) rarr mathbf(B) follows first order kinetics.The time take for 0.8 mole of A to produce 0.6 mole of B is 1 hour. What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of mathbf(B) .

The conversion of molecule A to B follows second order kinetics its rate equation for the second order reaction is rate = K[A]^2.If the concentration of A is increased to 4 times how will it affect the formation of B.

Choose the correct set of reactions which follow first order kinetics : (i) Thermal decomposition of HI on gold surface. (ii) Thermal decomposition of N_(2)O_(5)(g) at constant volume. (iii) Hydrogenation of ethene. (iv) Decomposition of NH_(3) on a hot Pt surface. (v) Thermal decomposition of SO_(2)Cl_(2)(g) at constant volume.

Write integrated rate equation for a first order reaction.

The gaseous reaction A(g) to 2B(g) + C(g) is found to be first-order respect to A. The reaction is started with p_A = 90 mmHg, the pressure after 10 min is found to be 180 mmHg. The rate constant of the reaction is

The reaction A(g) rarr B(g) + 2C(g) is a first order reaction with rate constant 2.772 xx 10^(-3) S^(-1) . Starting with 0.1 mole of A in 2 litre vessel, find the concentration of A after 250 sec when the reaction is allowed to take place at constant pressrue at 300 K.