Which statement is true of the internal energy of the system and its surroundings following a process in which AE = +65 kJ? Explain. a. The system and the surroundings both lose 65 kJ of energy. b. The system and the surroundings both gain 65 kJ of energy. c. The system loses 65 kJ of energy and the surroundings gain 65 kJ of energy. d. The system gains 65 kJ of energy and the surroundings lose 65 kJ of energy.

A 7.00kg piece of copper metal is heated from 18.4 °C to 357.3 °C. Calculate the heat absorbed (in kJ) by the metal (specific heat of copper is 0.385J/(g x°C)). a. 913335 kJ b. 727.51 kJ c. 1889 kJ d. 913.33 kJ

a. Determine whether energy as heat is evolved or required in the following process at constant pressure: N₂O4 (g) decomposes to form NO2 (g). Energy is required. O Energy is evolved. b. Determine whether work was done on the system or the system does work on the surroundings in the following process at constant pressure: N₂O4 (g) decomposes to form NO2 (g). O Work was done on the system. No work is done. O The system does work on the surroundings. c. Determine whether energy as heat is evolved or required in the burning of ethyne at constant pressure: 2 C₂ H₂ (g) + 5 O2 (g) → 4 CO2 (g) + 2 H₂O(g) Energy is required. O Energy is evolved. d. Determine whether work was done on the system or whether the system does work on the surroundings in the burning of ethyne at constant pressure: 2 C₂ H₂(g) + 5 O2 (g) → 4 CO2 (g) + 2 H₂O(g) Work was done on the system. O No work is done. O The system does work on the surroundings.

The specific heat capacity of silver is 0.24 J/°C.g. a. Calculate the energy required to raise the temperature of 143.0 g Ag from 268 K to 292 K. Energy = b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by 1.0°C (called the molar heat capacity of silver). Molar Heat Capacity= J/°C-mol c. It takes 1.18 kJ of energy to heat a sample of pure silver from 12.4°C to 15.4°C. Calculate the mass of the sample of silver. g Mass=