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Question

A car engine has a liquid coolant with a specific heat capacity of 3.75 J/(g•°C). The mass of coolant that will absorb 1.10 MJ of heat during a temperature rise from 22°C to 108°C is a.b kg.

A hot iron bar is lowered into a 400 g sample of water which is at a temperature of 24.0°C . If the water sample absorbs 2500 J of energy, the final temperature of the water is ab.c °C

1201 g of water is heated from 17 to 96 °C on the stove. The quantity of heat required is abc kJ.

An iron engine will absorb 1200000 J of heat when the temperature rises from 21.0 °C to 130.0 °C after it has started. The mass of the engine is ab.c kg.

2.00 kJ of heat flowed to a 97 g sample of a liquid solvent, causing a temperature increase from 15.15 °C to 21.49 °C. The specific heat capacity of the liquid a.bc J/g°C

Answer 1

q = mC∆T

q = heat = 1.10 MJ = 1.10x10⁶ J

m = mass = ?

C = specific heat = 3.75 J/gº

∆T= change in temperature = 108 - 22 = 86º

solving for m:

m = q / C∆T = 1.10x10⁶ J / (3.75 J/gº)(86º) = 3411 g = 3.4 kg

q = mC∆T

2500 J = (400 g)(4.184 J/gº)(∆T)

∆T = 1.5º

Final temperature = 22 + 1.5 = 23.5ºC

q = mCT

q = (1201 g)(4.184 J/gº)(79º) = 396,974 J = 397 kJ

q = mC∆T

m = q/C∆T = 1200000 J / (0.44 J/gº)(109º) = 25,021 g = 25.0 kg

q = mC∆T

C = q / m∆T = 2000 J / (97 g)(6.34º) = 3.25 J/gº