Question

Calculate the amount of heat (in loules) that must be added to 50.0 g of water to increase the temperature from 26.3C to 52.70. The specific heat of water is 4.18 J/g C An 50.0 g iron nail was heated in a blacksmith forge until it glowed cherry red. It was then dropped into a calorimeter containing 50.0 g of water at room temperature (21.5°C) and swirled gently until the temperature reached its maximum. The final temperature was 26.0 C. If the specific heat of iron is 0.1078 cal/g °C, what was the initial temperature of the metal? Remember, one eats a cow one bite at a time. This problem cannot be solved without using multiple steps.

Answer 1

1)

q = mc∆T

q amount of heat released it added

m is mass

c is specific heat capacity

∆T is temperature

Given that,

m = 50.0 g

c = 4.18 J/g.°C

∆T = 52.7 °C - 26.3 °C

∆T = 26.4 °C

q = 50.0 g × 4.18 J/g.°C × 26.4 °C

q = 5517.6 J

q = 5.52×10^3 J