A 3.68 g sample of solid gold is heated from 24 ºC to 34 ºC. How much energy

(in joules and calories) is required?

Thank you!

heat=mass*specificheat*dhangeinTemp

To calculate the amount of energy required, we can use the equation:

Q = mcΔT

Where:
Q is the amount of energy in joules,
m is the mass of the substance in grams,
c is the specific heat capacity of the substance (in joules per gram per degree Celsius), and
ΔT is the change in temperature in degrees Celsius.

First, let's calculate the amount of energy in joules.

Given:
m = 3.68 g
c (specific heat capacity of gold) = 0.129 J/g°C
ΔT = (34 °C - 24 °C) = 10 °C

Plugging these values into the equation, we get:

Q = (3.68 g) x (0.129 J/g°C) x (10 °C)
Q = 4.76 J

Therefore, the amount of energy required in joules is 4.76 J.

To convert this into calories, we can use the conversion factor:

1 calorie = 4.184 J

Therefore, the amount of energy required in calories is:

4.76 J x (1 cal / 4.184 J) ≈ 1.14 cal

Hence, the amount of energy required in calories is approximately 1.14 cal.