Calculate the energy required to heat 322.0g of ethanol from - 2.2°C to 19.6°C. Assume the specific heat capacity of ethanol under these conditions is 2.44·J·g-1K-1. Round your answer to 3 significant digits.

There is 17.1 kJ energy required

Explanation:

Step 1: Data given

Mass of ethanol = 322.0 grams

Initial temperature = - 2.2 °C = 273.15 - 2.2 = 270.95K

Final temperature = 19.6 °C = 273.15 + 19.6 = 292.75 K

Specific heat capacity = 2.44 J/g*K

Step 2: Calculate energy

Q = m*c*ΔT

⇒ m = the mass of ethanol = 322 grams

⇒ c = the specific heat capacity of ethanol = 2.44 J/g*K

⇒ ΔT = T2 - T1 = 292.75 - 270.95 = 21.8 K

Q = 322 * 2.44 * 21.8 = 17127.8 J = 17.1 kJ

There is 17.1 kJ energy required