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Chemistry
Zero order reaction
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:
$(A) 0.15mold{m^{ - 3}}$
$(B) 1.05mold{m^{ - 3}}$
$(C) 0.25mold{m^{ - 3}}$
$(D) 4.00mold{m^{ - 3}}$
Chemistry
Zero order reaction
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 $k = 2.5 \times {10^{ - 4}}mo{l^{ - 1}}L{s^{ - 1}}$ ?

Chemistry
Zero order reaction
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.

Chemistry
Zero order 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)

Chemistry
Zero order reaction
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) $- \dfrac{{{k_0}}}{{2.303}}$

Chemistry
Zero order reaction
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) $- 2.303k$

Chemistry
Zero order reaction
Explain zero order reaction with example.
Chemistry
Zero order reaction
${\text{k}}$ 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) $1 \cdot 0{\text{ M}}$

Chemistry
Zero order reaction
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.)${ { L }^{ 2 }mol }^{ -2 }{ s }^{ -1 }$

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