To determine which temperature pair is possible, we need to analyze how heat transfer would work between Block 1 and Block 2.

Initially:

• Block 1: 84°C
• Block 2: 150°C

Since Block 2 is hotter, heat would naturally transfer from Block 2 to Block 1, bringing them closer to an equilibrium temperature over time. The final temperatures should be between 84°C and 150°C, and they should be closer to each other than they initially were.

Let's examine each option:

1. 99°C for Block 1 and 135°C for Block 2: This is plausible. The temperatures are closer, and both are between 84°C and 150°C.
2. 32°C for Block 1 and 202°C for Block 2: This is impossible. The temperatures are outside the initial range (84°C to 150°C), and Block 2 has increased its temperature beyond the initial maximum, which violates conservation of energy.
3. 161°C for Block 1 and 161°C for Block 2: This is also impossible. Although the temperatures are equal (which suggests equilibrium), 161°C is higher than both original temperatures, which again violates conservation of energy.

Conclusion: The only feasible option is 99°C for Block 1 and 135°C for Block 2.

Would you like more details or have any questions?

Here are some related questions:

1. How does thermal equilibrium work between two objects?
2. What factors affect the rate of heat transfer between two objects?
3. How is conservation of energy applied in heat transfer scenarios?
4. Why can’t the temperature of an object increase without an external energy source?
5. What would happen if both blocks were initially at the same temperature?

Tip: In heat transfer, the final equilibrium temperature must always be between the initial temperatures of the objects involved, assuming no external energy input or loss.