Question

Linda 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 30.0 °C to a final temperature of 40.0 °C.

Which statement is true about the experiments?

The heat absorbed in Trial 1 is about 1,674 J greater than the heat absorbed in Trial 2.
The heat absorbed in Trial 1 is about 3,347 J greater than the heat absorbed in Trial 2.
The same amount of heat is absorbed in both the experiments because the heat absorbed depends only on the final temperature.
The same amount of heat is absorbed in both the experiments because the product of mass, specific heat capacity, and change in temperature are the same.

Answer 1

Answer:

$\boxed{\text{The heat absorbed in Trial 1 is about 3350 J greater than the heat absorbed in Trial 2}}$

Explanation:

The formula for the heat absorbed is

q = mCΔT

Trial 1

m = 30.0 g

ΔT = 40.0 – 0 = 40.0 °C

q₁ = 30.0 × 4.184 × 40.0 = 5020 J

Trial 2

m = 40.0 g

ΔT = 40.0 – 30.0 = 10.0 °C

q₂ = 40.0 × 4.184 × 10.0 = 1670 J

q₁ - q₂ = 5020 – 1670 = 3350  J

$\boxed{\text{The heat absorbed in Trial 1 is }\textbf{about 3350 J} \text{ greater than the heat absorbed in Trial 2}}$