Zero Order Reaction

Q. The half-life period of a zero order reaction is proportional to the initial concentration of reactants,

1. False
2. True

Q. { Q }10/58 The value of }K_c for the dissociation reaction is }}{H_2(g)=2H(g) is }1.2×10^{-43}} This equilibrium mixture contains

Q. The slope of Arrhenius Plot $\left(lnkv/s\frac{1}{T}\right)$ of first order reaction is $–5\times {10}^{3}K$. The value of $E_a$ of the reaction is. Choose the correct option for your answer.
[Given $R=8.314J{K}^{–1}mo{l}^{–1}$]

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Q. Consider the zero order reaction
$R\to P$
Starting with 4 moles of R in a one litre container, after half an hour only 1 mole of R is left unreacted. The value of k for the reaction is:

1. $0.1mol{L}^{-1}mi{n}^{-1}$
2. $0.3mol{L}^{-1}mi{n}^{-1}$
3. $1mol{L}^{-1}mi{n}^{-1}$
4. $0.4mol{L}^{-1}mi{n}^{-1}$

Q.

The rate constant of the reaction $A\to B$ is $0.6\times {10}^{-3}$ mole per second. If the concentration of B after 20 min is:

1. 1.08 M

2. 3.60 M

3. 0.36 M

4. 0.72 M

Q. Half-life period of a zero order reaction is

1. Proportional to initial concentration of reactants
2. Independent of initial concentration of reactants
3. Inversely proportional to initial concentration of reactants
4. Inversely proportional to square of initial concentration of reactants.

Q. The initial rate of zero order reaction of the gaseous reaction A(g) $\to$ 2B(g) is ${10}^{-2}$ M/min. If the initial concentration of A is 0.1 M, what would be the concentration of B after 60 sec?

1. 0.09 M
2. 0.01 M
3. 0.02 M
4. 0.002 M

Q.
A graph between $log{t}_{\frac{1}{2}}$ and $log\left[A_0\right]$ for a reaction at $27{}^{\circ }C$ is given above. From the graph, which of the following statement(s) is/are correct?
($t_{\frac{1}{2}}$= Half-life ; $\left[A_o\right]$ = Initial concentration)

1. The unit of k (rate constant) is the same as the rate of the reaction
2. The half-life is directly proportional to $\left[A_o\right]$
3. The half-life is independent of $\left[A_o\right]$
4. The slope of the graph between $\left[A_t\right]$ and $t$ is $–k$

Q. Is gay-lussacs law applicable in an incomplete reaction?

Q. Consider the reaction, 2Afor+ B(g)(g)2C(g)which Ko 350. If 0.001 mole of each of thereactants and product are mixed in a 2.0 L flaskthen the reaction quotient and the spontaneousdirection of the system will be

Q. For a reaction of order (n), the unit of the rate constant is :

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1. ${\text{mol}}^{1-n}{L}^{1-n}s$
2. ${\text{mol}}^{1-n}{L}^{2n}{s}^{-1}$
3. ${\text{mol}}^{1-n}{L}^{n-1}{s}^{-1}$
4. ${\text{mol}}^{1-n}{L}^{1-n}{s}^{-1}$

Q. Half-life period of a zero order reaction is

1. Proportional to initial concentration of reactants
2. Independent of initial concentration of reactants
3. Inversely proportional to initial concentration of reactants
4. Inversely proportional to square of initial concentration of reactants.

Q. The time required for $100\%$ completion of a zero order reaction is (a is the initial concentration and k is the rate constant)

1. $\frac{2k}{a}$
2. $\frac{a}{2k}$
3. $\frac{a}{k}$
4. $ak$

Q.

Match the following
Order of reaction Half-life period
1)1st order reaction a) $(k{a}_0{)}^{-1}$
2) Second order reaction b) $\frac{0.693}{k}$
3) Zero order reaction c) $\frac{a_0}{2k}$

1. 1-a , 2-b, 3-c
2. 1-b, 2-a, 3-c
3. 1-b, 2-c, 3-a
4. 1-c, 2-b, 3-a

Q. A first order reaction completes $50$% in $69.3$ minute. How much time it will take for $90$% completion?

Q. For reaction $A\to B$, rate constant of reaction at ${27}^{\circ }C$ is $1.2\times {10}^{-3}$ $M{s}^{-1}$. The only correct graph for the reaction is,

1. 
2. 
3. 
4. 

Q. The rate constant of the reaction $A\to B$ is $0.6\times {10}^{-3}\text{M/s}$. If the concentration of $A$ is $5\text{M}$, then concentration of $B$ after 20 minutes is :-

1. $0.36\text{M}$
2. $0.72\text{M}$
3. $1.08\text{M}$
4. $3.60\text{M}$