Please help me in my chem ;(

Question

The specific heat capacity of silver is 0.24 J/°C·g.

A. Calculate the energy required to raise the temperature of 154.0 g  from 268 K to 292 K.

Energy = _____  J

B. Calculate the energy required to raise the temperature of 1.0 mole of by 1.0°C (called the molar heat capacity of silver).

Molar Heat Capacity = ____  J/°C·mol

C. It takes 1.07 kJ of energy to heat a sample of pure silver from 12.9°C to 14.2°C. Calculate the mass of the sample of silver.

Mass =   g

Answer 1

q = mC∆T

q = heat energy = ?

m = mass = 154.0 g

C = specific heat = 0.24 J/g/deg

∆T = change in temperature = 292 - 268 = 24º

q = (154 g)(0.24 J/g/deg)(24 deg) = 887 J = 890 J (to 2 significant figures)

1.0 mole Ag x 107.9 g/mole = 107.9 g/mole x 0.24 J/g/deg = 25.9 J = 26 J/ºC/mol

q = mC∆T

q = 1.07 kJ = 1070 J

m = ?

C = 0.24 J/g/deg

∆T = 1.3 deg

m = q/C∆T = 1070 J/(0.24 J/g/deg)(1.3 deg)

m = 3429 g = 3430 g (to 3 significant figures)