College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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Steam at 100 °C is bubbled into 4.00 kg of water at 15 °C in a calorimeter cup. How much steam will have been added
when the water in the cup reaches 70 °C? (Ignore the effect of the cup.)
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- Q:33)arrow_forward(a) How much heat in joules is gained by the water?(b) How much heat in joules is lost by the metal?(c) What is the heat capacity of this piece of metal?arrow_forward2.00 kg of water has a volume of 2.00 x 10-3m3 when in the liquid state at 100 °C. When the water is completely changed from liquid to vapour at 100 °C, under a constant atmospheric pressure of1.01 x 105 Pa, the volume increases to 3.38 m3. (i) How much work is done against the atmosphere as the water changes into vapour?(ii) What is the change in the internal energy of the water during vaporization?arrow_forward
- (a) How much heat transfer (in kcal) is required to raise the temperature of a 0.650 kg aluminum pot containing 3.00 kg of water from 10.0°C to the boiling point and then boil away 0.600 kg of water? X kcal Enter a number. (b) How long (in s) does this take if the rate of heat transfer is 600 W (1 watt = 1 joule/second (1 W = 1 J/s))?arrow_forward1. (a) How much heat transfer is necessary to raise the temperature of a 0.26 -kg piece of ice from -20 °C to 130 °C, including the 20 kJ/s energy needed for phase changes? Specific heat of ice = 2.090 kJ/kg °C Specific heat of water = 4.186 kJ/kg °C Specific heat of steam = 1.520 kJ/kg °C Heat of fusion of water = 334 kJ/kg Heat of vaporization = 2256 kJ/kg (i) Heat needed to warm ice to 0 °C: Q₁: ✔KJ (ii) Heat needed to melt ice at 0 °C: Q₂: KJ (iii) Heat required to warm 0 °C water to 100 °C: Q3: KJ (iv) Heat required to vaporize water at 100 °C: Q4: KJ (v) Heat required to warm 100 °C vapor to 130 °C: Q5: KJ Total heat, Q: KJ (b) How much time is required for the entire process, assuming a constant 20.0 kJ/s rate of heat transfer? Total time, t: Sarrow_forwardA 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.arrow_forward
- (a) Compute the amount of heat (in J) needed to raise the temperature of 1.2 kg of water from its freezing point to its normal boiling point. __________ J (b) How does your answer to (a) compare to the amount of heat (in J) needed to convert 1.2 kg of water at 100°C to steam at 100°C? (The latent heat of vaporization of water at 100°C is 2.26 ✕ 106 J/kg.) Qa Qb =arrow_forwardOne strategy when on a diet is to drink ice water. The body must burn calories to warm the water from 32 °F to a body temperature of 98.6 °F. Assume a dieter drinks 2.4 kg (2.4 L) of ice water every day. How much energy, in Cal, does the dieter's body need to provide in order to warm the 2.4-L-water. (The specific heat of water is 4186 J/kg • °C; 1J = 0.000239 Cal.) Show your work.arrow_forward
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