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GradeZero Order Reaction

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The rate constant of a zero order reaction is $0.2 mol dm^{-3} h^{-1}$. If the concentration of the reactant after 30 minutes is $0.05 mol dm^{-3}$. Then its initial concentration would be:

$(A) 0.15mold{m^{ - 3}}$

$(B) 1.05mold{m^{ - 3}}$

$(C) 0.25mold{m^{ - 3}}$

$(D) 4.00mold{m^{ - 3}}$

$(A) 0.15mold{m^{ - 3}}$

$(B) 1.05mold{m^{ - 3}}$

$(C) 0.25mold{m^{ - 3}}$

$(D) 4.00mold{m^{ - 3}}$

The decomposition of $N{H_3}$ on the platinum surface is a zero order reaction. What are the rates of production of ${N_2}$ and ${H_2}$ if $k = 2.5 \times {10^{ - 4}}mo{l^{ - 1}}L{s^{ - 1}}$ ?

In a zero-order reaction:-

A. The rate constant has the unit ${\text{mol }}{{\text{L}}^{{\text{ - 1}}}}{{\text{s}}^{{\text{ - 1}}}}$

B. The rate is independent of the concentration of the reactants.

C. The half-life depends on the concentration of the reactants.

D. The rate is independent of the temperature of the reaction.

A. The rate constant has the unit ${\text{mol }}{{\text{L}}^{{\text{ - 1}}}}{{\text{s}}^{{\text{ - 1}}}}$

B. The rate is independent of the concentration of the reactants.

C. The half-life depends on the concentration of the reactants.

D. The rate is independent of the temperature of the reaction.

For the reaction of the Zeroth order, variation of log ${T_{50}}$ with log a (where ${T_{50}}$ is half-life period and a is the initial concentration) is given by:

A)

B)

C)

D)

A)

B)

C)

D)

For Zero order reactions, the linear plot was obtained for $\left[ A \right]$ vs $t$ . The slope of the line is equal to:

A) ${k_o}$

B) $ - {k_o}$

C) $\dfrac{{0.693}}{{{k_0}}}$

D) $ - \dfrac{{{k_0}}}{{2.303}}$

A) ${k_o}$

B) $ - {k_o}$

C) $\dfrac{{0.693}}{{{k_0}}}$

D) $ - \dfrac{{{k_0}}}{{2.303}}$

For a zero-order reaction, $A \to B$, a graph of rate vs time has slope equal to: (where $k = rate$)

(A) $k$

(B) $ - k$

(C) zero

(D) $ - 2.303k$

(A) $k$

(B) $ - k$

(C) zero

(D) $ - 2.303k$

Explain zero order reaction with example.

${\text{k}}$ for a zero-order reaction is $2 \times {10^{ - 2}}{\text{ }}{{\text{L}}^{ - 1}}{\text{ Se}}{{\text{c}}^{ - 1}}$. If the concentration of the reactant after ${\text{25 sec}}$ is $0 \cdot 5{\text{ M}}$, the initial concentration must have been:

(a) $0 \cdot 5{\text{ M}}$

(b) $1 \cdot 25{\text{ M}}$

(c) $12 \cdot 5{\text{ M}}$

(d) $1 \cdot 0{\text{ M}}$

(a) $0 \cdot 5{\text{ M}}$

(b) $1 \cdot 25{\text{ M}}$

(c) $12 \cdot 5{\text{ M}}$

(d) $1 \cdot 0{\text{ M}}$

The unit of rate constant for the zero-order reaction is:

A.)${ s }^{ -1 }$

B.)${ molL }^{ -1 }{ s }^{ -1 }$

C.)${ Lmol }^{ -1 }{ s }^{ -1 }$

D.)${ { L }^{ 2 }mol }^{ -2 }{ s }^{ -1 }$

A.)${ s }^{ -1 }$

B.)${ molL }^{ -1 }{ s }^{ -1 }$

C.)${ Lmol }^{ -1 }{ s }^{ -1 }$

D.)${ { L }^{ 2 }mol }^{ -2 }{ s }^{ -1 }$

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