The problem requires finding the interface temperature ($T_{int}$) between two cylindrical rods (A and B) made of different materials when they are joined end-to-end and subjected to different temperatures at their free ends. This is a problem of steady-state heat conduction.
Under steady-state conditions, the rate of heat transfer ($H$) is constant throughout the composite system. The heat flow rate through a cylindrical rod is given by the formula:
$H = \frac{KA \Delta T}{L}$
Where:
For the joined rods A and B, the rate of heat flow must be the same at the interface:
$H_A = H_B$
Using the heat flow formula:
$\frac{K_A A_A (T_A - T_{int})}{L_A} = \frac{K_B A_B (T_{int} - T_B)}{L_B}$
Since the cross-sectional area $A = \pi r^2$, we can substitute this in:
$\frac{K_A (\pi r_A^2) (T_A - T_{int})}{L_A} = \frac{K_B (\pi r_B^2) (T_{int} - T_B)}{L_B}$
Canceling $\pi$ from both sides yields:
$\frac{K_A r_A^2 (T_A - T_{int})}{L_A} = \frac{K_B r_B^2 (T_{int} - T_B)}{L_B}$
The problem provides the following information:
Rearranging the equation to group the ratios:
$\frac{K_A}{K_B} \times \frac{r_A^2}{r_B^2} \times \frac{L_B}{L_A} \times (T_A - T_{int}) = (T_{int} - T_B)$
Substitute the known ratios and temperatures into the equation:
$(\frac{1}{2}) \times (4) \times (1) \times (400 \text{ K} - T_{int}) = (T_{int} - 200 \text{ K})$
Simplify the left side:
$2 \times (400 - T_{int}) = (T_{int} - 200)$
Expand the terms:
$800 - 2 T_{int} = T_{int} - 200$
Rearrange to solve for $T_{int}$:
$800 + 200 = T_{int} + 2 T_{int}$
Combine terms:
$1000 = 3 T_{int}$
Calculate the final value:
$T_{int} = \frac{1000}{3}$ K
$T_{int} \approx 333.33$ K
The calculated interface temperature is $\frac{1000}{3}$ K.
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 _________ $\text{J}$.
