The heat of combustion of propane, C3H8, is 2220 kJ/mol. The specific heat of copper is 0.385 J/g°C. How many grams of propane must be burned to raise the temperature of a 10.0 kg block of copper from 25.0°C to 65.0°C, assuming none of the heat is lost to the surroundings?

Explanation:

q = (mass) (temp change) (specific heat)

q = (10000 g) (40 °C) (0.385 J/g⋅°C) = 154000 J = 154 kJ

154 kJ / 2220 kJ/mol = 0.069369369 mol

0.069369369 mol times 44.0962 g/mol = 3.06 g (to three sig figs)

answer choice 4

can you attach the

atomic mass = 39

number of neutrons = 20

number of protons= 19

electronic configuration = 1s2 2s2 2p6 3s2 3p6 4s1

the number of electron in first shell = 2

number of electrons in n=3 shell = 8