A very hot piece of metal is placed in 200 mL of water. Thewater is initially at 20°C and heats up to 25 °C. Rememberingthat water has a specific heat of 1 cal/(g* C), how much heatdid the water gain?Q =unitThe metal had a mass of 218 grams and began at a temperature122 °C. Assuming that iron lost all of the heat the water gainedand also reached a final temperature of 25 °C, what is itsspecific heat capcityC =cal/(g*° C)

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A very hot piece of metal is placed in 200 mL of water. The water is initially at 20°C and heats up to 25 °C. Remembering that water has a specific heat of 1 cal/(g* C), how much heat did the water gain? Q = unit

A very hot piece of metal is placed in 200 mL of water. The water is initially at 20°C and heats up to 25 °C. Remembering that water has a specific heat of 1 cal/(g* C), how much heat did the water gain? Q = unit

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)...

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Measurement of specific heat of metals Aluminum Cupper Mass of inner cup of calorimeter mcal, g 50 50 Specific heat of calorimeter Ccal, cal/(g °C) Specific heat of water Cw, cal/(g °C) 0.217 0.217 1.00 1.00 Mass of metal Mm, g 80 140 Mass of inner cup + water mcal + Mw, g 220 240 Mass of water Mw, g 170 190 Initial temperature of calorimeter and water to, °C Initial temperature of metal tm, °C 22 22 100 100 Final equilibrium temperature tr, °C 30 26 Thermal energy gain by calorimeter and water Qgain, cal Specific heat of metal Cm, cal/(g °C) Standard specific heat of metal Cst , cal/(g °C) 0.217 0.093 |% error Thermal energy lost = Thermal energy gained Thermal energy Q = cmAt %3D %3D Specific heat C |Thermal energy lost by metal = Thermal energy gained by (water + calorimeter) %3D EmMm(tm-tf)=(ccatMeat +CwMw)(tp- to) %3D (Ccaimcal+ Cymw)(tf- to). Gm = %3D Mm(tm - t;) |
2.2 kg of ice (solid phase of water) at -10°C is heated under atmospheric pressure. Answer the following questions. Use the following values for your calculation. specific heat of ice: 2.1 kJ/(kg °C) specific heat of water: 4.2 kJ/(kg °C) specific heat of vapor: 2.0 kJ/(kg °C) latent heat of fusion: 334 kJ/kg latent heat of vaporization: 2260 kJ/kg How much heat is required to change the phase of the liquid water to vapor? How much heat is required to raise the temperature of vapor to 200°C?
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