The half-life of $2 $ sample are $0.1 $ and $ 0.4 $ seconds. Their respective concentration are $200 $ and  $ 50 $ respectively. What is the order of the reaction

For a reactions $A + B \to $product, it was found that rate of reaction increases four times if concentration of $ ‘A’$  is doubled, but the rate of reaction remains unaffected. If concentration of $‘B’ $ is doubled. Hence, the rate law for the reaction is

For a general reaction $A \to B$, plot of concentration of $A$ vs time is given in figure. Answer the following question on the basis of this graph.

$(i)$ What is the order of the reaction ?

$(ii)$ What is the slope of the curve ?

$(iii)$ What are the units of rate constant ?

If a reaction has the experimental rate expression rate $= K [A]^2[B]$, if the concentration of $A$ is doubled and the concentration of $B$ is halved, the what happens to the reaction rate

What is the order of a reaction which has a rate expression rate $ = K{[A]^{3/2}}{[B]^{ - 1}}$

In a chemical reaction $A$ is converted into $B$ . The rates of reaction, starting with initial concentrations of $A$ as $2 \times {10^{ - 3}}\,M$ and $1 \times {10^{ - 3}}\,M$ , are equal to $2.40 \times {10^{ - 4}}\,M{s^{ - 1}}$ and $0.60 \times {10^{ - 4}}\,M{s^{ - 1}}$ respectively. The order of reaction with respect to reactant $A$ will be