The specific heat of silver is 0.24 . How many joules of energy are needed to warm 4.37 g of silver from 25.0C to 27.5C?

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The question asks: The specific heat of silver is 0.24 [J/g·°C]. How many joules of energy are needed to warm 4.37 g of silver from 25.0°C to 27.5°C?

First, determine the temperature change: ΔT = 27.5°C − 25.0°C = 2.5°C.

Next, use the formula q = m × c × ΔT, where m is mass in grams and c is specific heat in J/(g·°C).

Compute the product step by step:
- m × c = 4.37 g × 0.24 J/(g·°C) = 1.0488 J/°C
- (m × c) × ΔT = 1.0488 J/°C × 2.5°C = 2.622 J

Thus the energy required is approximately 2.62 J.

Now evaluate each option:
- Option 1: 2.62 J — This matches the calculated value using the correct units and inputs, so it is correct.
- Option 2: 0.14 J — This is too small by about a factor of 19. It would result from either a much smaller mass, a much smaller ΔT, or a smaller c than given; none of these align with the problem data.
- Option 3: 45.5 J — This would require a much larger product m × c × ΔT; for example, using kilograms instead of grams or a far larger ΔT, which is inconsistent with the provided values.
- Option 4: 0.022 J — This is also far too small and corresponds to an even smaller energy change than the second option, not reconcilable with the given mass, c, and ΔT.

In summary, only the 2.62 J option is consistent with q = m c ΔT using m = 4.37 g, c = 0.24 J/(g·°C), and ΔT = 2.5°C.

Chemistry (H) - Varnold - Preparatory Academy - 2nd Semester - 2024/2025 2025 Thermochemistry Practice Test

The specific heat of silver is 0.24 . How many joules of energy are needed to warm 4.37 g of silver from 25.0C to 27.5C?

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