Question

Shane performed the following trials in an experiment. Trial 1: Heat 30.0 grams of water at 0 °C to a final temperature of 40.0 °C. Trial 2: Heat 40.0 grams of water at 10.0 °C to a final temperature of 40.0 °C. Which statement is true about the experiments?
A. The same amount of heat is absorbed in both the experiments because the product of mass, specific heat capacity, and change in temperature are equal for both.

B. The same amount of heat is absorbed in both the experiments because the heat absorbed depends only on the final temperature.

C. The heat absorbed in Trial 2 is about 3,674 J greater than the heat absorbed in Trial 1.

D. The heat absorbed in Trial 2 is about 5,021 J greater than the heat absorbed in Trial 1.

Answer 1

Answer:

A. The same amount of heat is absorbed in both the experiments because the product of mass, specific heat capacity, and change in temperature are equal for both.

Explanation:

• The amount of heat absorbed by water (Q) can be calculated from the relation:

Q = m.c.ΔT.

where, Q is the amount of heat absorbed by water,

m is the mass of water,

c is the specific heat capacity of water (c = 4.186 J/g °C),

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

• For trial 1:

m = 30.0 g, c = 4.18 J/g °C, ΔT = 40.0 °C – 0.0 °C = 40.0 °C

∴ Q = m.c.ΔT = (30.0 g)(4.18 J/g °C)(40.0 °C) = 5023 J.

• For trial 2:

m = 40.0 g, c = 4.18 J/g °C, ΔT = 40.0 °C – 10.0 °C = 30.0 °C

∴ Q = m.c.ΔT = (40.0 g)(4.18 J/g °C)(30.0 °C) = 5023 J.

• So, the right choice is:

A. The same amount of heat is absorbed in both the experiments because the product of mass, specific heat capacity, and change in temperature are equal for both.

Answer 2

Answer:

its a

Explanation:

i took it on the exam