Calculate the amount of heat loss for a 5.08 cm thick glass wall when its temperature changes from 20.0 °C to 40.0°C in 60.0 seconds. The length of the wall is 98.5 cm and its width is 45.3 cm. O 1,090,000 calories O 2, 110 calories 90,900 calories O 886,000 calories 9,380 calories

Calculate the amount of heat loss for a 5.08 cm thick glass wall when its temperature changes from 20.0 °C to 40.0°C in 60.0 seconds. The length of the wall is 98.5 cm and its width is 45.3 cm. O 1,090,000 calories O 2, 110 calories 90,900 calories O 886,000 calories 9,380 calories

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

12 Assume Lake Huron contains 3.60 x 10-2 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 12.8°C to 23.6°C? 1.627e24 From the density of water and the volume, what is the mass of the water? What is specific heat? How is it related to the energy input, mass, and temperature change? Use it to solve for the energy. Be careful with units. 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? yr
0.0550 kg piece of glass is heated to an unknown temperature and dropped into a calorimeter containing 0.150 kg of water at 12.0 °C. The glass and the water reach a final temperature of 18.0 °C. What is the initial temperature of the glass?
A gas exerts a pressure of one atmosphere at standard temperature (273 K). At what value should the temperature (in °C) be adjusted to for the gas to exert a pressure of 4.0 atmosphere keeping the volume unaltered? (Hint : Pressure varies directly with absolute temperature) 1092 °C O - 205 °C 819 °C 68.3 °C
600g of ice at -8°C is put inside a calorimeter filled with 4000 g water initially at 20 °C. What is the final temperature of the system? c water = 4.186 J/g°C c of ice = 2.093 J/g°C Hf = 334 J/g
A person wants to cool down her bath water so she does so by adding 5.0 Kg of ice at 0°C to 75.0 Kg of water at 70°C. What would the final temperature of the water be ? Lf = 333 KJ/Kg & cH2O =4186 J/Kg°C
A 31.5 g glass thermometer reads 23.6°C before it is placed in 135 mL of water. When the water and thermometer come to equilibrium, the thermometer reads 41.8°C. What was the original temperature of the water? Ignore the mass of fluid inside the glass thermometer. chapter 8:heat and thermodynamics
A block of copper with mass 0.600 kg is heated to 400. degrees Celsius from 260. degrees Celsius. The specific heat capacity of copper is 387 J/ (kg°C). The heat absorbed by the copper block is 2.88 E5 J 3.25 E4 J 6.04 E5 J 9.29 E4 J
How much thermal energy/heat is required to raise 2.3 kg of lead from 300°C to 1800°C? Use Table 1 p281 and Table 1 p291 to help you. O 1.8 x 10°J O 2. 5 x 10°J O8.2 x 10³J O4.5 x 10°J x 10°J
A student measures the following data in a calorimetry experiment designed to determine the specific heat of aluminum. (Do not assume atmospheric pressure.) Initial temperature of water and calorimeter: 70°C Mass of water: 0.400 kg Mass of calorimeter: 0.040 kg Specific heat of calorimeter: 0.63 kJ/kg · °c Initial temperature of aluminum: 26.5°C Mass of aluminum: 0.200 kg Final temperature of mixture: 65.9°C Use these data to determine the specific heat of aluminum. J/kg · °C
A 0.422 g food sample is used to raise the temperature of 14.656 g of water by 45.2 celsius. How many food Calories (kilocalories) of energy does the food contain per gram?
In a physics lab, students are conducting an experiment to learn about the heat capacity of different materials. The first group is instructed to add a number of 1.50 g pellets made of lead, at a temperature of 92.0°C, to 305 g of water at 16.0°C. A second group is given the same number of 1.50 g pellets as the first group, but these are now aluminum pellets. Assume that no heat is lost to or gained from the surroundings for either group. (a) If the final equilibrium temperature of the lead pellets and water is 25.0°C, how many whole pellets did the first group use in the experiment? The specific heat of lead is 0.0305 kcal/(kg · °C). pellets (b) Will the final equilibrium temperature for the second group be higher, lower, or the same as for the first group? The specific heat of aluminum is 0.215 kcal/(kg · °C). O higher O lower O the same (c) What is the equilibrium temperature of the aluminum and water mixture for the second group? °C
How much heat energy must be removed from 0.10 kg of oxygen with a temperature of 22 °C in order for the oxygen to liquefy at -183 °C? (Co = 913 J/kg°C, Ly = 2.13 x 105 J/kg and oxygen liquefies as -183 °C) O 5 x 10^4 J O 9 x 10^4 J O 1 x 10^4 J O 4 x 10^4J