For a chemical reaction $A \rightarrow B$,it was found that the concentration of $B$ increases by $0.2 \, mol \, L^{-1}$ in $30 \, min$. The average rate of the reaction is $...... \times 10^{-1} \, mol \, L^{-1} \, h^{-1}$. (Nearest integer)
- A$1$
- B$2$
- C$3$
- D$4$
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Similar Questions
For the following reaction in aqueous solution,what happens to the rate of reaction if $HCl$ is added?
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$
$NH_2NO_{2(aq)} + OH^-_{(aq)} \to NHNO^-_{2(aq)} + H_2O_{(l)}$
$NHNO^-_{2(aq)} \to N_2O_{(aq)} + OH^-_{(aq)}$
Easy
View SolutionIdentify the correct expression for the rate of the following reaction: $2 N_2 O_{5(g)} \rightarrow 4 NO_{2(g)} + O_{2(g)}$
Which one of the following equations is correct for the reaction $N_{2(g)} + 3H_{2(g)} \longrightarrow 2NH_{3(g)}$?
From the concentrations of $C_{4}H_{9}Cl$ (butyl chloride) at different times given below,calculate the average rate of the reaction:
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
$t/s$ $0$ $50$ $100$ $150$ $200$ $300$ $400$ $700$ $800$ $[C_{4}H_{9}Cl]/mol\ L^{-1}$ $0.100$ $0.0905$ $0.0820$ $0.0741$ $0.0671$ $0.0549$ $0.0439$ $0.0210$ $0.017$
$C_{4}H_{9}Cl + H_{2}O \rightarrow C_{4}H_{9}OH + HCl$
during different intervals of time.
| $t/s$ | $0$ | $50$ | $100$ | $150$ | $200$ | $300$ | $400$ | $700$ | $800$ |
| $[C_{4}H_{9}Cl]/mol\ L^{-1}$ | $0.100$ | $0.0905$ | $0.0820$ | $0.0741$ | $0.0671$ | $0.0549$ | $0.0439$ | $0.0210$ | $0.017$ |
Difficult
View SolutionFill in the blanks:
$(a)$ The rate of reaction ....... as the concentration of reactant decreases.
$(b)$ The rate of reaction ....... as the concentration of product increases.
$(a)$ The rate of reaction ....... as the concentration of reactant decreases.
$(b)$ The rate of reaction ....... as the concentration of product increases.
Medium
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