A container holds 2.0 g of Helium at a pressure of 6.0 atm. (a) How much heat is required to increase the temperature by 100°C at constant volume? (b) How much will the temperature increase if this amount of heat energy istransferred to the gas at constant pressure?
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A container holds 2.0 g of Helium at a pressure of 6.0 atm. (a) How much heat is required to increase the temperature by 100°C at constant volume? (b) How much will the temperature increase if this amount of heat energy istransferred to the gas at constant pressure?
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- A small office building with well-insulated walls and containing 600 m3 of air at 305 K is heated at constant pressure (atmospheric). Consider air to be an ideal diatomic gas. (a) Determine the energy (in kJ) required to increase the temperature of the air in the building by 1.70°C.(b) Determine the mass (in kg) this amount of energy could lift through a height 2.30 m.Assume Lake Superior contains 1.20 ✕ 1013 m3 of water, and assume the water's density is that of water at 20°C and 1 atm. (a) How much energy (in J) is required to raise the temperature of that volume of water from 14.0°C to 21.2°C? J (b) How many years would it take to supply this amount of energy by using a power of 1,400 MW generated by an electric power plant? yrIf you have 6 moles of a diatomic ideal gas (such as oxygen or nitrogen), how much heat is required to raise the temperature of this gas from 261.5K to 282K if the volume of the gas remains constant during the heating?
- 4.00 Litres of hydraulic oil is placed in a cylinder with a movable piston, on which a heavy block is placed. The hydraulic oil pressure is maintained at 2.45x105 Pa and the temperature of the oil is raised by 45K. The oil is in the liquid phase and expands by a small amount 1.2x10-3m3. Calculate the work done on the oil and the change in internal energy of the oil. The specific heat capacity of hydraulic oil is 2300J/(kg.K) and its density is 800kg/m3A 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.In an insulated vessel, 239 g of ice at 0°C is added to 635 g of water at 15.0°C. (Assume the latent heat of fusion of the water is 3.33 x 10° J/kg and the specific heat is 4,186 J/kg · °C.) (a) What is the final temperature of the system? °C (b) How much ice remains when the system reaches equilibrium?
- A vertical cylinder with a heavy piston contains air at 300 K. The initial pressure is 2.00 × 105 Pa, and the initial volume is 0.350 m3. Take the molar mass of air as 28.9 g/mol and assume CV = 5/2 R. (a) Find the specific heat of air at constant volume in units of J/kg ? °C. (b) Calculate the mass of the airin the cylinder. (c) Suppose the piston is held fixed. Find the energy input required to raise the temperature of the air to 700 K. (d) What If? Assume again the conditions of the initial state and assume the heavy piston is free to move. Find the energy input required to raise the temperature to 700 K.In a container of negligible mass, 0.150 kg of ice at 0°C and 0.0950 kg of steam at 100°C are added to 0.200 kg of water that has a temperature of 50.0°C. (a) If no heat is lost the environment and the pressure in the container is constant at 1.00 atm, find the final temperature of the system. (b) At the final temperature, how many kilograms are there of ice, how many of liquid, and how many of steam.