Question

The initial temperature of a bomb calorimeter is 28.50°C. When a chemist carries out a reaction in this calorimeter, its temperature decreases to 27.45°C. If the calorimeter has a mass of 1.400 kg and a specific heat of 3.52 J/(gi°C), how much heat is absorbed by the reaction? Use . 140 J 418 J 1,470 J 5,170 J

Answer 1

When 40.0 mL of 1.00 M H2SO4 is added to 80.0 mL of 1.00 M NaOH at 20.00°C in a coffee cup calorimeter, the temperature of the aqueous solution increases to 29.20°C. If the mass of the solution is 120.0 g and the specific heat of the calorimeter and solution is 4.184 J/g • °C, how much heat is given off in the reaction? (Ignore the mass of the calorimeter in the calculation.)

Use q equals m C subscript p Delta T..

4.62 kJ

10.0 kJ

14.7 kJ

38.5 kJExplanation:

Answer 2

5,170 J.

Step-by-step explanation:

• The amount of heat absorbed by the reaction = the amount of heat released from the calorimeter.

• the amount of heat released from the calorimeter (Q) can be calculated from the relation:

Q = m.c.ΔT.

where, Q is the amount of heat released from the calorimeter (Q = ??? J),

m is the mass of the calorimeter (m = 1.4 kg = 1400.0 g),

c is the specific heat capacity of the calorimeter (c = 3.52 J/g °C),

ΔT is the temperature difference (final T - initial T) (ΔT = 27.45 - 28.50 = - 1.05°C).

∵ Q = m.c.ΔT.

∴ Q = m.c.ΔT = (1400.0 g)(3.52 J/g °C)(- 1.05°C) = - 5174.0 J ≅ - 5,170 J.

∴ The amount of heat absorbed by the reaction = 5,170 J.