CP1 Chapter 10 Energy In Class Practice

+96 joules

5.0 g of copper was heated from 20°C to 70°C. How much energy was used to heat Cu? (Specific heat capacity of Cu is 0.092 cal/g °C)

0.61 J/(g∙°C)

A 155 g sample of an unknown substance was heated from 15°C to 40°C. In the process, the substance absorbed 569 calories of energy. What is the specific heat of the substance?

1.34 J/(g∙°C)

A 32-gram substance needs to be heated from 13℃ to 89℃ using 3265 J of energy in order to boil. What is the specific heat of the substance?

134°C

A 4.50 g coin of copper absorbed 45 calories of heat. What was the final temperature of the copper if the initial temperature was 25°C? The specific heat of copper is 0.092 cal/g°C.

2.43 J/(g∙°C)

A 41 gram substance needs to be heated from 52℃ to 57℃ using 498 J of energy in order to melt. What is the specific heat of the substance?

31.9 °C

A 85 g coin of copper releases 54 calories of heat. The specific heat of copper is 0.092 cal/g°C. What was the final temperature of the copper if the initial temperature was 25°C?

123°C

A 95 g bar of copper absorbed 4500 calories of heat. The specific heat of copper is 0.092 cal/g°C. What was the change in temperature of the bar of copper?

1504 g

A sample of metal is cooled until it is solid, from 3000℃ to 2700℃, losing 56.4 kJ of heat. The specific heat of the metal is 0.125 J/g℃. What is the mass of the sample?

109 g

A sample of molten lead is cooled from 3000℃ to 1700℃, losing 18.2kJ of heat. The specific heat of iron is 0.128 J/g℃. The melting point of iron is 1750℃. What is the mass of the sample?

+17.5 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: 2N₂O (g) → 2NO (g) + N₂ (g) N₂ (g) + O₂ (g) → 2NO (g) ΔH = +180.7 J 2N₂O (g) → O₂ (g) + 2N₂ (g) ΔH = -163.2 J

-196 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: 2SO₂ (g) + O₂ (g) → 2SO₃ (g) 2S (s) + 3O₂ (g) → 2SO₃ (g) ΔH = -790 J S (s) + O₂ (g) → SO₂ (g) ΔH = -297 J

-59.0 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: 3 Fe₂O₃ (s) + CO (g) → CO₂ (g) + 2 Fe₃O₄ (s) Fe₂O₃ (s) + 3CO (s) → 2Fe (s) + 3CO₂ (g) ΔH = -28.0 J 3Fe (s) + 4CO₂ (s) → 4CO (g) + Fe₃O₄ (s) ΔH = +12.5 J

-293.8 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: 4NO (g) → 2NO₂ (g) + N₂ (g) N₂ (g) + O₂ (g) → 2NO (g) ΔH = +180.7 J 2NO (g) + O₂ (g) → 2NO₂ (g) ΔH = -113.1 J

+571.6 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: CaCO₃ (s) → CaO (s) + C (s) + O₂ (g) CaCO₃ (s) → CaO (s) + CO₂ (g) ΔH = 178.1 J C (s) + O₂ (g) → CO₂ (g) ΔH = -393.5 J

+355 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: IF₅ (g) → IF₃ (g) + F₂ (g) IF (g) + F₂ (g) → IF₃ (g) ΔH = -390 J IF (g) + 2F₂ (g) → IF₅ (g) ΔH = -745 J

+180.6 J

Calculate ΔH in joules for the following reaction given the data below: Goal Reaction: N₂ (g) + O₂ (g) → 2NO (g) N₂ (g) + 2O₂ (g) → 2NO₂ (g)ΔH = 66.4 J 2NO (g) + O₂ (g) → 2NO₂ (g) ΔH = -114.2 J

-9.23 kJ

For the reaction S(s) + O₂ (g) → SO₂ (g), ΔH =-296 kJ per mole of SO₂ formed. Calculate the quantity of heat released when 1.00 g of sulfur is burned in oxygen.

-148 kJ

For the reaction S(s) + O₂ (g) → SO₂ (g), ΔH =-296 kJ per mole of SO₂. Calculate the quantity of heat released when 0.501 mole of sulfur is burned in air.

-26.9 kJ

For the reaction S(s) + O₂ (g) → SO₂ (g), ΔH =-296 kJ per mole of SO₂. What quantity of energy is required to form 5.83 g of SO₂?

7.96 g

Given the following equation, calculate the grams of C₃H₈ you would need to provide 369 kJ of heat. C₃H₈(g) + 5O₂ (g) → 3CO₂ (g) + 4H₂O (g), ∆H=-2043 kJ

-1.90 kJ

Given the following equation, what is the enthalpy change per 1.00 grams of nitrogen monoxide? 2NO (g) +O₂ (g) → 2NO₂ (g), ∆H=-114 kJ

-665 kJ

Given the following equation, what is the enthalpy change to burn 35.8 g of NH₃? 4NH₃(g) + 3O₂ (g) → 2N₂ (g) + 6H₂O (g), ∆H=-1267 kJ

+119 joules

How much heat is absorbed by 15g granite boulder as energy from the sun causes its temperature to change from 10°C to 29°C? (Specific heat capacity of granite is 0.1 cal/gºC)

-6832 J

How much heat is released when 23 g of water at 96°C cools to 25°C? The specific heat of water is 1 cal/g°C.

1.08 J/(g∙°C)

If a 3.1g ring is heated using 14.4 calories, its temperature rises 17.9°C. Calculate the specific heat capacity of the ring.

1.21 J/(g∙°C)

The temperature of a sample of iron with a mass of 10.0 g changed from 50.4°C to 25.0°C with the release of 74 calories of heat. What is the specific heat of iron?

246.6 g

The temperature of a sample of water increases from 20°C to 46.6°C as it absorbs 6560 calories of heat. What is the mass of the sample? (Specific heat of water is 1.0 cal/g °C)

7.03 J/(g∙°C)

What is the specific heat of an unknown substance if a 2.50 g sample releases 21 calories as its temperature changes from 25°C to 20°C?