How much energy is required to raise the temperature of 5.0 g of silver from 298 K to
334 K?

43.2J

Explanation:

Q = m × c × ∆T

Where:

Q = amount of energy

m = mass (grams)

c = specific heat capacity

∆T = change in temperature

Mass = 5.0g

Specific heat capacity of Silver (Ag) = 0.240 J/g°C

We need to convert the temperature from Kelvin (K) to °C

Initial temperature = 298 - 273 = 25°C

Final temperature = 334 - 273 = 61°C

Q = 5 × 0.240 × (61°C - 25°C)

Q = 1.2 × 36

Q = 43.2J

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