A mixture containing 21.4 g of ice (at exactly 0.00 ∘C) and 75.3 g of water (at 80.2 ∘C) is placed in an insulated container.

Assuming no loss of heat to the surroundings, what is the final temperature of the mixture?

A mixture containing 21.4 of ice (at exactly 0.00) and 75.3 of water (at 80.2) is placed in an insulated container.

Assuming no loss of heat to the surroundings, what is the final temperature of the mixture?

41.9 ∘C

46.9 ∘C

44.7 ∘C

32.6 ∘C

Question

Bryan

Chemistry

5 March, 01:08

A mixture containing 21.4 g of ice (at exactly 0.00 ∘C) and 75.3 g of water (at 80.2 ∘C) is placed in an insulated container.

Assuming no loss of heat to the surroundings, what is the final temperature of the mixture?

A mixture containing 21.4 of ice (at exactly 0.00) and 75.3 of water (at 80.2) is placed in an insulated container.

Assuming no loss of heat to the surroundings, what is the final temperature of the mixture?

41.9 ∘C

46.9 ∘C

44.7 ∘C

32.6 ∘C

+2

Answers (1)

Know the Answer?

Chelsea Mack · Answer 1

Heat gained in a system can be calculated by multiplying the given mass to the specific heat capacity of the substance and the temperature difference. In a mixture it should be that heat gained is equal to the heat removed. We calculate as follows

Q1 = - Q2

21.4 (T2-0.00) = - 75.3 (T2 - 80.2)

T2 = 62.45