Question

The rate constant of the reaction $A\to 2B$ is $1.0\times {10}^{-3}mol{lit}^{-1}{min}^{-1}$, if the initial concentration of B after 100 minutes:

• A. $0.1mol{lit}^{-1}$
• B. $0.2mol{lit}^{-1}$
• C. $0.9mol{lit}^{-1}$
• D. $1.8mol{lit}^{-1}$

Answer 1

The correct option is B $0.2mol{lit}^{-1}$

Rate constant $k=1\times {10}^{-3}mol/lit.min$

$A\to 2B$

After 100 minutes,

reactant used$=k\times 100$

$=0.1mole/litersA:B=1:2$

$\therefore$ Product formed=$2\times$ reactants used

$=0.1\times 2$

$=0.2mol/L$

Hence, the correct option is $B$