This problem involves Newton's Law of Cooling, which describes how the rate of heat loss of a body is proportional to the temperature difference between the body and its surroundings.
The integrated form of Newton's Law of Cooling is given by:
$ \ln\left(\frac{T_1 - T_s}{T_2 - T_s}\right) = kt $Where:
We are given the first cooling interval:
Plugging these values into the formula:
$ \ln\left(\frac{60 - 25}{50 - 25}\right) = k \times 10 $ $ \ln\left(\frac{35}{25}\right) = 10k $ $ \ln\left(\frac{7}{5}\right) = 10k $So, the cooling constant $k$ is:
$ k = \frac{1}{10} \ln\left(\frac{7}{5}\right) $Now, we need to find the temperature ($T_3$) after the next 10 minutes. The second interval starts from $T_2 = 50^\circ C$ and lasts for $t = 10$ minutes.
Using the formula again:
$ \ln\left(\frac{T_2 - T_s}{T_3 - T_s}\right) = kt $Substitute the value of $k$ and the known temperatures:
$ \ln\left(\frac{50 - 25}{T_3 - 25}\right) = \left(\frac{1}{10} \ln\left(\frac{7}{5}\right)\right) \times 10 $ $ \ln\left(\frac{25}{T_3 - 25}\right) = \ln\left(\frac{7}{5}\right) $Equating the terms inside the logarithm:
$ \frac{25}{T_3 - 25} = \frac{7}{5} $Solve for $T_3$:
$ 25 \times 5 = 7 \times (T_3 - 25) $ $ 125 = 7T_3 - 175 $ $ 7T_3 = 125 + 175 $ $ 7T_3 = 300 $ $ T_3 = \frac{300}{7} $ $ T_3 \approx 42.857^\circ C $The calculated temperature $T_3$ is approximately $42.857^\circ C$. Comparing this with the given options, the closest value is $43^\circ C$. Therefore, the temperature of the body after the next 10 minutes will be approximately $43^\circ C$.
10 mole of an ideal gas is undergoing the process shown in the figure. The heat involved in the process from $P_1$ to $P_2$ is $\alpha \text{ Joule}$ ($P_1 = 21.7 \text{ Pa}$ and $P_2 = 30 \text{ Pa}, C_v = 21 \text{ J/K.mol}, R = 8.3 \text{ J/mol.K}$). The value of $\alpha$ is _______.

A thermodynamic system is taken through the cyclic process ABC as shown in the figure. The total work done by the system during the cycle $ABC$ is _________ $\text{J}$.

10 mole of an ideal gas is undergoing the process shown in the figure. The heat involved in the process from $P_1$ to $P_2$ is $\alpha \text{ Joule}$ ($P_1 = 21.7 \text{ Pa}$ and $P_2 = 30 \text{ Pa}, C_v = 21 \text{ J/K.mol}, R = 8.3 \text{ J/mol.K}$). The value of $\alpha$ is _______.

A thermodynamic system is taken through the cyclic process ABC as shown in the figure. The total work done by the system during the cycle $ABC$ is _________ $\text{J}$.
