A 5.63 g sample of solid gold is heated from 21.0 ºC to 32.0 ºC. How much energy (in J and cal) is required?

According to q formula:

q = M C ΔT

when q is the energy required in Joule

M is the mass per kilogram=5.63 g / 1000 = 0.00563 Kg

C is the specific heat capacity of the gold J (Kg-K) = 125.6 J (Kg-K) (should be given in the specific heat capacity table)

ΔT is the change in the temperature = (32 - 21) = 11 C°

∴q = 0.00563 * 125.6 * 11 = 7.78 J = 1.86 Cal