Question 1 The specific heats of Lead and Gold are both is 0

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?