How much heat energy is required to raise the temperature of 0.358 kg of copper from 23.0 ∘C to 60.0 ∘C? The specific heat of copper is 0.0920 cal/(g⋅∘C) .

In order to calculate how much heat is needed to raise the temperature you need to use the formula q =mass x specific heat x (final temperature- initial temperature) where q represents heat being absorbed or released. Before you begin you would convert kg to g because the specific heat is measure in g. So you would set up the equation as q = 358 g x .092 x (60-23 degrees Celsius) which would give you 1218.6

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dsdrajlin dsdrajlin · Answer 2 · 2020-01-13T21:51:31+01:00

Answer:

1.22 × 10³ cal

Explanation:

Given data

Mass of Cu (m): 0.358 kg = 358 g

Initial temperature: 23.0°C

Final temperature: 60.0°C

Change in the temperature (ΔT): 60.0°C - 23.0°C = 37.0°C

Specific heat of Cu (c): 0.0920 cal/g.°C

We can calculate the heat (Q) required to raise the temperature of 0.358 kg of copper from 23.0°C to 60.0°C using the following expression.

Q = c × m × ΔT

Q = (0.0920 cal/g.°C) × 358 g × 37.0°C

Q = 1.22 × 10³ cal