The specific heat capacity of gold is 0.13 J/g°C. How many calories of energy are needed to warm 0.570 g of gold from 30.0°C to 39.5°C?
A) 0.70 cal
B) 0.17 cal
C) 1.2 cal
D) 2.9 cal
E) 23 cal

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of energy needed to warm up the gold.

q = m * c * ΔT

where q is the amount of energy, m is the mass of the gold, c is the specific heat capacity of gold, and ΔT is the change in temperature (final temperature - initial temperature).

Plugging in the given values:

q = (0.570 g) * (0.13 J/g°C) * (39.5°C - 30.0°C)

q = 0.570 * 0.13 * 9.5 = 0.77 J

Now, we need to convert from joules to calories. There are 4.184 J in 1 cal, so:

q = 0.77 J * (1 cal / 4.184 J)

q = 0.184 cal

Therefore, the answer is C) 1.2 cal (rounded to 1 decimal place).

The Specific Heat Capacity of Gold Is 0