In an insulated container, you combine hot metal with ice. The ice starts at -20 degrees C. The copper starts at 900 degrees C. When 15 kg of the copper is combined with an unknown amount of ice, the system reaches equilibrium as soon as all of the ice has boiled to become steam. The way to solve this is to add up all of the heat transfer terms and set them equal to zero EQ = 0 How many Q terms are there for this problem?

In an insulated container, you combine hot metal with ice. The ice starts at -20 degrees C. The copper starts at 900 degrees C. When 15 kg of the copper is combined with an unknown amount of ice, the system reaches equilibrium as soon as all of the ice has boiled to become steam. The way to solve this is to add up all of the heat transfer terms and set them equal to zero EQ = 0 How many Q terms are there for this problem?

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

A2.9 kg lump of aluminum is heated to 95°C and then dropped into 10.0 kg of water at 5.0°C. Assuming that the lump-water system is thermally isolated, what is the system's equilibrium temperature? Assume the specific heats of water and aluminum are 4186 and 900 J/kg-K, respectively. Number i Units
A 155 g copper bowl contains 230 g of water, both at 20.0°C. A very hot 300 g copper cylinder is dropped into the water, causing the water to boil, with 4.05 g being converted to steam. The final temperature of the system is 100°C. Neglect energy transfers with the environment. (a) How much energy (in calories) is transferred to the water as heat? 8.6 X kcal (b) How much energy (in calories) is transferred to the bowl? 55 X kcal (c) What is the original temperature of the cylinder? 553.6 X °C Did you use the idea of conservation of energy? That is, did you equate the sum of the energy transfers to zero? For the bowl and cylinder, did you substitute the expression relating an energy transfer, the specific heat, the mass, and the temperature change? For the water, did you use the same expression to get the water to the boiling point? Did you also include an expression for the heat of vaporization? Did you use the given final temperature for each of the three materials?
Rubbing your hands together warms them by converting work into thermal energy. a. If a woman rubs her hands a total of 19 times (forward and backwards count separately), at a distance of 7.75 cm per rub, and with an average frictional force of 39 N, what is the temperature increase of her hands, in degrees Celsius? The mass of tissues warmed is only 0.100 kg, mostly in the palms and fingers, and the heat capacity of her hands is 3500 J/(kg⋅°C).
In an effort to stay awake for an all-night study session, a student makes a cup of coffee by first placing a 200 W electric immersion heater in 0.400 kg of water. How much heat must be added to the water to raise its temperature from 21.0°C to 77.0°C? Express your answer in joules. IVE ΑΣΦ Q = Submit Part B t = Request Answer Submit How much time is required? Assume that all of the heater's power goes into heating the water. Express your answer in seconds. OF 15. ΑΣΦ ? Request Answer J ? S Re
A steel rod (p=7860 kg/m³) has a length of 3.75 m. It is bolted at both ends between immobile supports. Initially there is no tension in the rod, because the rod just fits between the supports. Find the tension that develops when the rod loses 3190 J of heat. Number ! Units N
The initial temperature of 150 g of ice is -20°C. The spe-cific heat capacity of ice is 0.5 cal/g.C° and water's is1 cal/g•C°. The latent heat of fusion of water is 80 cal/g.a.How much heat is required to raisethe ice to 0°C andcompletely melt the ice?b. How much additional heat is required to heat the water(obtained by melting the ice) to 25°C?C.What is the total heat that must be added to convert the80 g of ice at-20°C to water at +25°C?d. Can we find this total heat simply by computing howmuch heat is required to melt the ice and adding theamount of heat required to raise the temperature of 80 gof water by 45°C? Explain
J Problem 8.10*. (a) For the human body, what is the rate of heat transfer by conduction through the body's tissue k = 0.200m.K with the following conditions: the tissue thickness is 3.00 cm, the change in temperature is 2.00°C, and the skin area is 1.50 m². [20.0 W] (b) What fraction of your daily caloric intake goes into warming your body in this situation? [20.7%]