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4. Heat transfer: q = mass x Cs x ΔT and –qreaction = +qsolution

a. A piece of metal with a mass of 8.6 g was heated to 100.0°C and dropped into a coffee cup

calorimeter containing 402.4 g of water at 25.0°C. If the temperature of the water and the

metal at thermal equilibrium is 26.4°C, what is the specific heat of this metal in J/g°C?

b. How much heat energy must be added in order to boil a liter of water (initial temperature of

24.0°C) in a 1.0 kg copper pot? The specific heat capacity of water is 4.184 J/g°C and the

specific heat capacity of copper is 0.385 J/g°C.

c. A 50.0 g piece of iron (Tinitial = 225°C) and a 50.0 g piece of gold (Tinitial = 25.0°C) are

brought into contact with each other. Assuming no heat is lost to the surroundings, calculate the

temperature of the two metals when they reach thermal equilibrium. The specific heat

capacity of iron = 0.449 J/g°C and the specific heat capacity of gold = 0.128 J/g°C.

d. A 100.0 mL sample of 0.300 M NaOH is mixed with a 100.0 mL sample of 0.305 M HNO3 in

a coffee cup calorimeter. If both solutions were initially at 25.0°C and the maximum

temperature of the resulting mixture was 28.5°C. Find the heat of the reaction, qreaction, in

joules and report the molar heat of reaction, ΔHreaction, in kJ/mole. The density of both

solutions is 1.00 g/mL and heat capacity is the same as water: 4.184 J/g°C.

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