Be sure to answer all parts. The height of Niagara Falls on the American side is 51 m. (a) Calculate the potential energy of 1.0 g of water at the top of the falls relative to the ground level. Hint: The work done in ascending is given by mgh, where m is the mass (in kg), g is the gravitational acceleration (9.8 m/s? ), and h is the height (in meters). J (b) What is the speed of the falling water if all the potential energy is converted to kinetic energy? m/s (c) What would be the increase in temperature of the water if all the kinetic energy were converted to heat?

How much work (energy) is required to lift a 173 g object by a height of 71.0 feet? The earth's gravitational constant is g = 9.80 m/s2.

A 1.70-mol sample of hydrogen gas is heated at constant pressure from 306 K to 414 K. (a) Calculate the energy transferred to the gas by heat. (Enter your answer to at least two decimal places.)  kJ(b) Calculate the increase in its internal energy. (Enter your answer to at least two decimal places.)  kJ(c) Calculate the work done on the gas.  kJ

The distance between Sherbrooke and Montreal is 137km. However, a car driving between the two points travels 156km. Of these distances, which one is analogous to a state function?

and 2 Enthalpy #1.30 enoindice pled TT 2010 2D49.bs 22) When 1 mole of Fe2O3(s) reacts with H₂(g) to form Fe(s) and H2O(g) according to the following equation, 98.8 kJ of energy are absorbed. (6 Fe2O3(s) + 3 H2(g) → 2 Fe(s) + 3 H₂O(g) (pp) (20/d4 (pm) $40 D Reaclanis 13:48 SH Products endothermic, A endothermic, B (2) exothermic, A exothermic, B nad W (21 Enthalpy MOMS. Reactants Products (A) (B) Is the reaction endothermic or exothermic, and which of the enthalpy diagrams above represents grow olor and to noin (01 this reaction? SH GH TH A HOMH X HILD 08.10 Page 6 of 8

A gas expands from 287 mL to 959 mL at a constant temperature. Calculate the work done (in joules) by the gas if it expands (a) against a vacuum. W = J (b) against a constant pressure of 4.00 atm. W = J

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.508-g sample of benzil (C14H1002) in a bomb calorimeter containing 1060. g water. The temperature increases from 24.70 °C to 27.80 °C. The specific heat capacity of water is 4.184 J gl°C1. The combustion enthalpy is -6784 k]/mol benzil. C14H1002(s) + 31/2 02(g) →14 CO2(g) + 5 H20(I) A,H° = -6784 kJ/mol %3D Calculate the heat capacity of the calorimeter. heat capacity of calorimeter = J/C

5.00 × 10−2 mol KOH and an excess of hydrochloric acid are combined in 100.0 mL of water initially at 25.0 °C, leading to a final measured temperature of 31.1 °C. (a) What is the heat flow for the water in the calorimeter, qH2O, in Joules? (b) Assuming the calorimeter constant Ccal = 50.0 J °C , what is the heat flow for the calorimeter, qcal, in Joules? (c) What is the amount of heat given off by the reaction, qrxn, in Joules? (d) What is the molar enthalpy of the neutralization reaction (shown below) as measured in the calorimeter, ∆H◦ rxn in kilojoules per mole? H3O + (aq) + OH– (aq) → 2H2O (l)

Calculate the molar heat capacity (cm) for Iron (Fe). cFe = 0.451 J/(g•oC) Express your answer 3 significant figures, and without the units.

Calculate AE and determine whether the process is endothermic or exothermic for the following cases: (1) q = 0.123 kJ and w = - 230 J (2) A system releases 66.1 kJ of heat to its surroundings while the surroundings to 44.0 kJ of work on the system.