Question

For the following question, enter the correct numerical value up to TWO decimal places. If the numerical value has more than two decimal places, round-off the value to TWO decimal places. (For example: Numerical value 5 will be written as 5.00 and 2.346 will be written as 2.35) The entropy of a sample of a certain substance increases by \(0.836\,\text{J K}^{-1}\) on adding reversibly \(0.3344\,\text{J}\) of heat at constant temperature. The temperature of the sample is _____ K

Hint:

For reversible heat transfer at constant temperature, use \( \Delta S = \dfrac{Q_{\text{rev}}}{T} \).

Answer 1

Correct Answer: 0.4

Step 1: For a reversible process at constant temperature, the change in entropy is given by \[ \Delta S = \frac{Q_{\text{rev}}}{T}. \]
Step 2: Given: \[ \Delta S = 0.836\,\text{J K}^{-1}, \quad Q_{\text{rev}} = 0.3344\,\text{J}. \]
Step 3: Rearranging the formula to find temperature: \[ T = \frac{Q_{\text{rev}}}{\Delta S}. \]
Step 4: Substituting values, \[ T = \frac{0.3344}{0.836} = 0.40\,\text{K}. \] Hence, the temperature of the sample is \[ \boxed{0.40\,\text{K}}. \]