A piece of iron (CsFe = 0.45 J/g·⁰C) with a mass of 4.45 g at temperature of 101.0 oC is dropped into an insulated calorimeter containing 50.0 g of water at 22.00 oC. What will be the final temperature of the water?

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Chemistry

1 November, 23:40

A piece of iron (CsFe = 0.45 J/g·⁰C) with a mass of 4.45 g at temperature of 101.0 oC is dropped into an insulated calorimeter containing 50.0 g of water at 22.00 oC. What will be the final temperature of the water?

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Carlo Pruitt · Answer 1

22.75 ⁰C.

Explanation:

The amount of heat added to a substance (Q) can be calculated from the relation:

Q = m. c.ΔT.

where, Q is the amount of heat added,

m is the mass of the substance,

c is the specific heat of the substance,

ΔT is the temperature difference (final T - initial T).

∵ The amount of heat released by Fe = the amount of heat absorbed by water

∴ - (m. c.ΔT) released by Fe = (m. c.ΔT) absorbed by water.

- (4.45 g) (0.45 J/g·⁰C) (final T - 101.0 ⁰C) = (50.0 g) (4.186 J/g·⁰C) (final T - 22.0 ⁰C)

- 2.0025 final T + 202.2525 = 209.3 final T - 4604.

209.3 final T + 2.0025 final T = 202.2525 + 4604

211.3025 final T = 4806.2525.

final T = 4806.2525/211.3025 = 22.75 ⁰C.