How much heat is required to raise the temperature of 91.5 g of water from its melting point to its boiling point? Express your answer numerically in kilojoules. Can someone answer this for me in decimal form?

38.2836 kJ

Explanation:

Mass = 91.5g

Initial Temperature = melting point = 0 C = 273 K (upon converting to kelvin)

Final Temperature = Boiling point = 100 C = 373 K

Heat = ?

They are related by the equation;

H = mCΔT

ΔT = Final - Initial Temperature = 373 - 273 = 100 K

C = specific heat capacity = 4.184 J /gK

H = 91.5 * 4.184 * 100

H = 38283.6 J

To convert to kilojoules, divide by 1000. This leaves us with;

H = 38283.6 / 1000 = 38.2836 kJ

fe 55.85 g/mol and h2o 18.02 g/mol.