Question 1

The specific heats of Lead and Gold are both is 0.128 J/g°C. Which of the following statements is not true?

Select one:

a. When 10.0 g of lead is heated from 25°C to 35°C, it gains128 J of heat

b. When 10.0 g of gold is heated from 25°C to 35°C, it gains128 J of heat

c. Gold and Lead have the same molar heat capacity

d. None of the statements are false

e. Lead has the higher molar heat capacity

Question 2

Calculate ΔH for the reaction

4 NH3 (g) + 5 O2 (g) →4 NO (g) + 6 H2O (g), from the following data:

N2 (g) + O2 (g) →2 NO (g) ΔH = -181 kJ

N2 (g) + 3 H2 (g) →2 NH3 (g) ΔH = -92.0 kJ

2H2(g) +O2(g) →2H2O(g) ΔH = -484 kJ

Question 3

The combustion of propane produces heat according to the equation:

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) ΔH° = is –2044 kJ

How much heat will be evolved if 2.20g of propane is combusted?

Question 4

A 20.0 g piece of a metal with specific heat of 0.900 J/g.0C at 98.0 0C dropped into 50.0 g water in a calorimeter at 20.0 0C. The specific heat of water is 4.18 J/g.0C Calculate the final equilibrium temperature of the mixture

Question 5

A gas heated and it absorbs 100 kJ of heat. It expand doing 25 kJ of work. What is the internal energy change of the gas?

Question 6

Calculate the standard enthalpy of formation of propane, C3H8(g), given that ΔH°f[CO2(g)] = –394 kJ/mol and

ΔH°f[H2O(l)] = –242 kJ/mol, and the following thermochemical equation

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) ΔH° = is –2044 kJ

Question 7

Given that the molecular formula of sand is SiO2 and that its specific heat is 0.84 J/g°C, its molar heat capacity is

Question 8

Calculate the standard enthalpy change for the following reaction given that the ΔHf° of benzene, C6H6(l) is 49 kJ/mol, the ΔH°f of CO2(g) = –394 kJ/mol and ΔH°f of H2O(g) = –242 kJ/mol:

2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) ΔH° = ?

Question 9

The standard enthalpy of formation, ΔHf°, of which of the following is zero at room temperature (298K)?

Select one:

a. All of the above

b. CO2(g)

c. Br2(g)

d. H2O(l)

e. Br2(l)

Question 10

A 47.3 g sample of an alloy was heated to 90.00 oC and then dropped into a beaker containing 90.0 g of water at a temperature of 25.00 oC. The temperature of the water rose to a final temperature of 28.00 oC. The specific heat of water is 4.184 J/goC. What is the specific heat capacity of the alloy?

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