The rate constant for a first order reaction is 4.606 10-3 s-1. The time required to reduce 2.0 g of the reactant to 0.2 g is:

Correct answer: (A) 500 s. Answer: (A) 500 s Solution: For a first order reaction t=2.303/k [R]_0/[R]. Here [R]_0=2.0 g, [R]=0.2 g, so [R]_0/[R]=10 and 10=1. Therefore t= 2.3034.606 10-3 1=2.303/0.004606=500 s.

NEET 2020 · ChemistryIntegrated ratePrevious Year Question

The rate constant for a first order reaction is $4.606 \times 1 0^{- 3} s^{- 1}$ . The time required to reduce $2.0 g$ of the reactant to $0.2 g$ is:

Answer: (A) $500 s$ . \textbf{Answer:} (A) $500 s$ \textbf{Solution:} For a first order reaction $t = \frac{2.303}{k} lo g \frac{[ R ] _{0}}{[ R ]}$ .

A. $500 s$ ✓
B. $1000 s$
C. $100 s$
D. $200 s$

Correct Answer

(A) $500 s$

Solution & Explanation

\textbf{Answer:} (A) $500 s$ \textbf{Solution:} For a first order reaction $t = \frac{2.303}{k} lo g \frac{[ R ] _{0}}{[ R ]}$ . Here $[R]_{0} = 2.0 g$ , $[R] = 0.2 g$ , so $\frac{[ R ] _{0}}{[ R ]} = 10$ and $lo g 10 = 1$ . Therefore $t = \frac{2.303}{4.606 \times 1 0 ^{- 3}} \times 1 = \frac{2.303}{0.004606} = 500 s$ .

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The rate constant for a first order reaction is 4.606×10−3 s−1. The time required to reduce 2.0 g of the reactant to 0.2 g is:

Solution & Explanation

More NEET PYQ solutions

The rate constant for a first order reaction is $4.606 \times 1 0^{- 3} s^{- 1}$ . The time required to reduce $2.0 g$ of the reactant to $0.2 g$ is: