The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J)is required to raise the temperature of 10.0 mL of bromine from 25.00 °C to 27.30 °C? The density of liquid bromine: 3.12 g/mL.

Question

Quizplus · Accepted Answer

First, we need to calculate the mass of the bromine sample:
mass = density * volume = 3.12 g/mL * 10.0 mL = 31.2 g
Then, we can use the formula Q = m * c * ΔT, where Q is the heat required, m is the mass, c is the specific heat, and ΔT is the change in temperature.
Q = 31.2 g * 0.226 J/g-K * (27.30 °C - 25.00 °C) = 16.2 J
Therefore, the answer is B)16.2 J.

The Specific Heat of Liquid Bromine Is 0