Instantaneous rate of a reaction is $$ - {1 \over 2}{{d[x]} \over {dt}} = - {{d[y]} \over {dt}} = {1 \over 2}{{d[z]} \over {dt}}$$, identify the reaction.

Half life for a first order reaction is 6.93 hour. What is the time required for 80% completion of the reaction?

If concentration of reactant '$$A$$' is increased by 10 times the rate of reaction becomes 100 times. What is the order of reaction, if rate law is, rate $$=k[A]^x$$ ?

A first order reaction has rate constant $$1 \times 10^{-2} \mathrm{~s}^{-1}$$. What time will, it take for $$20 \mathrm{~g}$$ or reactant to reduce to $$5 \mathrm{~g}$$ ?