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The rate constant of a reaction with a v...

The rate constant of a reaction with a virus is `3.3xx10^(-4)S^(-1)`. Time required for the virus to become `75%` inactivated is

A

`35 mi n`

B

`70 mi n`

C

`105 mi n`

D

`17.5 mi n`

Text Solution

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The correct Answer is:
To solve the problem of determining the time required for a virus to become 75% inactivated, we will use the formula for the half-life of a first-order reaction. Here are the steps: ### Step 1: Understand the Reaction Order The problem states that the reaction is first-order. For a first-order reaction, the time required for a certain percentage of the reactant to be consumed can be calculated using the first-order rate equation. ### Step 2: Identify Given Values - Rate constant (k) = \(3.3 \times 10^{-4} \, \text{s}^{-1}\) - Percentage inactivated = 75% - Remaining concentration = 100% - 75% = 25% ### Step 3: Set Up the Equation The formula for the time \( t \) required for a first-order reaction is given by: \[ t = \frac{2.303}{k} \log\left(\frac{[A]_0}{[A]}\right) \] Where: - \([A]_0\) = initial concentration (100%) - \([A]\) = remaining concentration (25%) ### Step 4: Substitute the Values Substituting the known values into the equation: \[ t = \frac{2.303}{3.3 \times 10^{-4}} \log\left(\frac{100}{25}\right) \] ### Step 5: Calculate the Logarithm Calculate the logarithm: \[ \log\left(\frac{100}{25}\right) = \log(4) \] Using the known value: \[ \log(4) \approx 0.602 \] ### Step 6: Substitute the Logarithm Value Now substitute the logarithm back into the equation: \[ t = \frac{2.303}{3.3 \times 10^{-4}} \times 0.602 \] ### Step 7: Perform the Calculation Calculate the time: 1. Calculate \( \frac{2.303}{3.3 \times 10^{-4}} \): \[ \frac{2.303}{3.3 \times 10^{-4}} \approx 6970.3 \] 2. Multiply by \( 0.602 \): \[ t \approx 6970.3 \times 0.602 \approx 4201 \, \text{seconds} \] ### Step 8: Convert Seconds to Minutes To convert seconds into minutes: \[ \text{Minutes} = \frac{4201}{60} \approx 70.02 \, \text{minutes} \] ### Final Answer The time required for the virus to become 75% inactivated is approximately **70 minutes**. ---

To solve the problem of determining the time required for a virus to become 75% inactivated, we will use the formula for the half-life of a first-order reaction. Here are the steps: ### Step 1: Understand the Reaction Order The problem states that the reaction is first-order. For a first-order reaction, the time required for a certain percentage of the reactant to be consumed can be calculated using the first-order rate equation. ### Step 2: Identify Given Values - Rate constant (k) = \(3.3 \times 10^{-4} \, \text{s}^{-1}\) - Percentage inactivated = 75% ...
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