Lake Erie contains roughly 4.00 ✕ 1011 m3 of water. How much energy is required to raise the temperature of that volume of water from 18.0°C to 21.0°C? How many years would it take to supply this amount of energy by using the 1,400-MW exhaust energy of an electric power plant?

You have a spherical heater, outside diameter = 3.40 cm, immersed in a container of water. In order to keep the water in the container heated to a constant temperature of 35.0°C you adjust the temperature of the spherical heater. You reach a steady-state condition when the surface temperature of the spherical heater is at 79.0°C. Assuming the electrical efficiency of the heater is 100.0%, calculate the power required by the heater (i.e., calculate q). Ignore radiation.

A pot containing 1.70 kg of water is sitting on a hot stove, and the water is stirred violently by a mixer that does 6.40 kJ of mechanical work on the water. The temperature of the water rises by 4.00°C. What quantity of heat flowed into the water from the stove during the process? The specific heat of water is 4.186 kJ/kg·K.

46:56 WLwvimdGI A 52-kg package is lifted to the top shelf in a storage bin that is 4 m above the ground floor. How much increase in potential energy does the package get? O 1504733.118 Ib-ft 1937.104 BTU O 2040.48 kJ O 2.04 kJ

A woman expends 95 kJ of energy in walking a kilometer. The energy is supplied by the metabolic breakdown of food intake and has a 35 percent efficiency. If the woman drives a car over the same distance, how much energy is used if the car gets 8.8 km per liter of gasoline (approximately 20 mi/gal)? The density of gasoline is 0.71 g/mL, and its enthalpy of combustion is 49 kJ/g. Enter your answer in scientific notation.   Compare the efficiencies of the two processes.    kJ (driving)/ kJ (walking)

Suppose 9.30 x 105 J of energy are transferred to 2.00 kg of ice at 0°C. (a) Calculate the energy required to melt all the ice into liquid water. (b) How much energy remains to raise the temperature of the liquid water? (c)Determine the final temperature of the liquid water in Celsius.

A 160 g copper bowl contains 120 g of water, both at 25.0°C. A very hot 420 g copper cylinder is dropped into the water, causing the water to boil, with 5,00 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy is transferred to the water as heat? (b) How much to the bowl? (c) What is the original temperature of the cylinder? The specific heat of water is 1 cal/g-K, and of copper is 0.0923 cal/g-K. The latent heat of vaporization of water is 539 Cal/kg.

Required information A 3.00-kg object is initially moving northward at 15.0 m/s. Then a force of 15.0 N, toward the east, acts on it for 2.00 s. At the end of the 2.00 s, what is magnitude of the object's final velocity?

A container holding 4.20 kg of water at 20.0°C is placed in a freezer that is kept at -20.0°C. The water freezes and comes to thermal equilibrium with the interior of the freezer. What is the minimum amount of electrical energy required by the freezer to do this if it operates between reservoirs at temperatures of 20.0°C and –-20.0°C? (Latent heat of fusion of ice = capacity of water = 4186 J/(kg K), specific heat capacity of ice = 2100 J/(kg K)). 333,700 J/ kg, specific heat kJ