Law of mass action Questions in English

(B) According to the law of mass action,the rate of a chemical reaction at a given temperature is directly proportional to the product of the molar concentrations of the reactants,each raised to the power equal to its stoichiometric coefficient in the balanced chemical equation.

(A) The $Law \ of \ mass \ action$ states that the rate of a chemical reaction is directly proportional to the product of the active masses (molar concentrations) of the reacting substances.
Active mass is defined as the molar concentration of the substance,i.e.,$Active \ mass = [Concentration]$.

(A) The Law of Mass Action was proposed by $Cato \ Guldberg$ and $Peter \ Waage$ in $1864$.
It states that the rate of a chemical reaction is directly proportional to the product of the active masses (or molar concentrations) of the reactants,each raised to the power of its stoichiometric coefficient.

(D) The law of mass action states that the rate of a chemical reaction is directly proportional to the product of the active masses of the reactants.
Active mass is defined as the molar concentration of the substance,expressed in $mol \ L^{-1}$.

(D) According to the Law of Mass Action,the rate of a chemical reaction is directly proportional to the product of the active masses (molar concentrations) of the reactants,each raised to the power of its stoichiometric coefficient in the balanced chemical equation.

(D) The rate of a chemical reaction is directly proportional to the concentration of the reactants,which is referred to as the $Active \ mass$ of the substance. This is based on the $Law \ of \ Mass \ Action$,which states that the rate of a reaction is proportional to the product of the active masses of the reactants raised to the power of their stoichiometric coefficients. Therefore,the correct option is $(D)$.

(C) According to the Law of Mass Action,the rate of a chemical reaction at a constant temperature is directly proportional to the product of the molar concentrations of the reactants,each raised to the power of its stoichiometric coefficient in the balanced chemical equation.
Therefore,the correct option is $(C)$.

(B) The rate law for the reaction is given by $\text{Rate} = k[A]^2[B]^1$.
When the active mass of $A$ is doubled,the new rate becomes $\text{Rate}' = k[2A]^2[B]^1$.
$\text{Rate}' = k \times 4[A]^2[B]^1 = 4 \times \text{Rate}$.
Therefore,the rate of reaction increases $4$ times.

(A) Active mass is defined as the molar concentration,which is the number of moles per liter of volume.
Number of moles of $NH_3$ = $\frac{\text{Given mass}}{\text{Molar mass}}$ = $\frac{8.5 \ g}{17 \ g \ mol^{-1}} = 0.5 \ mol$.
Active mass = $\frac{\text{Number of moles}}{\text{Volume in liters}} = \frac{0.5 \ mol}{1 \ L} = 0.5 \ mol \ L^{-1}$.

(A) The $Law \ of \ mass \ action$ states that the rate of a chemical reaction is directly proportional to the product of the active masses (or molar concentrations) of the reactants,each raised to the power of its stoichiometric coefficient in the balanced chemical equation. Therefore,the correct option is $A$.

(D) The molar mass of $HI$ is $1 + 127 = 128 \ g/mol$.
Number of moles of $HI = \frac{\text{mass}}{\text{molar mass}} = \frac{64}{128} = 0.5 \ mol$.
Active mass is defined as molarity,which is $\frac{\text{moles}}{\text{volume in liters}}$.
Active mass $= \frac{0.5 \ mol}{2 \ L} = 0.25 \ mol/L$.