Thermochemistry Review

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron. Show all work and proper units.

• 0.46 J/g°C

• 0.15 J/g°C

• 1.25 J/g°C

• 0.90 J/g°C

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C? Show all work and proper units.

• 297 J

• 150 J

• 500 J

• 33 J

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NGSS.HS-PS3-4

To what temperature will a 50.0-g piece of glass raise if it absorbs 5275 joules of heat and its specific heat capacity is 0.50 J/g°C? The initial temperature of the glass is 20.0°C.

• 231°C

• 120°C

• 75°C

• 50°C

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• 1.8 J/g°C

• 0.30 J/g°C

• 2.5 J/g°C

• 0.90 J/g°C

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100.0 mL of 4.0°C water is heated until its temperature is 37°C. If the specific heat of water is 4.18 J/g°C, calculate the amount of heat energy needed to cause this rise in temperature.

• 13,800 J

• 8,200 J

• 21,500 J

• 3,900 J

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6. 25.0 g of mercury is heated from 25°C to 155°C, and absorbs 455 joules of heat in the process. Calculate the specific heat capacity of mercury.

• 0.14 J/g°C

• 0.20 J/g°C

• 0.10 J/g°C

• 0.30 J/g°C

What is the specific heat capacity of silver metal if 55.00 g of the metal absorbs 47.3 calories of heat and the temperature rises from 50°C to 75°C?

• 0.14 J/g°C

• 0.25 J/g°C

• 0.09 J/g°C

• 0.33 J/g°C

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NGSS.HS-PS3-4

If a sample of chloroform is initially at 25°C, what is its final temperature if 150.0 g of chloroform absorbs 1.0 kilojoules of heat, and the specific heat of chloroform is 0.96 J/g°C?

• 32°C

• 29°C

• 38°C

• 27°C

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NGSS.HS-PS3-4

How many joules of heat are given off when 5.0 g of water cool from 75ºC to 25ºC (specific heat of water = 4.184 J/g·ºC)? Would this be an endothermic or exothermic reaction?

• q = -1,046 J, Exothermic

• q = 1,046 J, Endothermic

• q = -418 J, Exothermic

• q = -2,092 J, Endothermic

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NGSS.HS-PS3-4

How many joules of energy are absorbed by 100 g of water heated from 20 ºC to 40 ºC? (specific heat of water = 4.184 J/g·ºC)? Would this be an endothermic or exothermic reaction?

• q = 8,368 J, Endothermic

• q = 4,184 J, Exothermic

• q = 2,000 J, Endothermic

• q = 10,000 J, Exothermic

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