50 g of copper is heated to increase its temperature by 100C. If the same amount of heat is applied to 10 g of water, its rise in temperature would be (Specific heat of copper = 420 J/k °C) O 8°C O 5°C O 7°C O 6°C

A 117-g cube of ice at 0°C is dropped into 1.0 kg of water that was originally at 79°C. What is the final temperature of the water after the ice has melted?

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

A 365-g sample of an unknown (nongaseous) material experiences a 16.0°C increase in temperature after absorbing 9.93 ✕ 103 J of energy. (a) What is the specific heat of this material? J/(kg · °C)(b) Which substance listed in the specific heat and molar specific heat table best matches the specific heat of this unknown material? mercurysilver    brassgraniteglassaluminumwoodseawater

Steam at 100°C is added to ice at 0°C. (a) Find the amount of ice melted and the final temperature when the mass of steam is 11 g and the mass of ice is 58 g.  ?g  ?°C (b) Repeat with steam of mass 3.7 g and ice of mass 58 g. ? g  ?°C

What quantity of heat (in J) would be required to convert 2.65 mol of a pure substance from a liquid at 40.0 °C to a gas at 113.0 °C? A Cliquid = 1.45 J/mol °C Tboiling = 88.5 °C Cgas = 0.65 J/mol °C AHvaporization = 1.23 kJ/mol

a sample of beryllium (1820J/kgC) at 20 degrees celsius into a 0.22kg glass beaker also at 20 degrees celsius. Water of mass 0.3kg and temperature 80 degrees celsius is poured over the beryllium. If the thermal equilibrium temperature of the closed system is 40 degrees celsius, what is the mass of the beryllium?

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