low temperature experiment, you have a puck of water ice (m1 = 10 g) in liquid n

Question

low temperature experiment, you have a puck of water ice (m1 = 10 g) in liquid nitrogen at a temperature of 77 K. You take the puck out the nitrogen and put it in a glass (mg = 400 g) which starts at room temperature (about 300 K). What is the final temperature of water glass system? Assume that the system is well insulated from its surroundings Does the ice melt? The water is heated to 500K How much heat goes into the water? What state is it in?(Hint: think about what volume it should have ) Assume the water's initial temperature is that calculated in part a, Of 280 K, and that the pressure is constant at 1 atmosphere.

Explanation / Answer

m_ice c_ice (deltaT) + m L = m_glass c_glass (deltaT) -------------------------------------------------------------------------------- ==> 10 * 2.11 * (273 - 77) + 10*334 + 10 * 4.18*(Tf - 273) = 400 * 0.84 * (300 - Tf) --------------------------------------------------------------------------- ==> Tf = 277 Kelvins ----------------------------------------------------------------------------------------------------------------------------------------------------------- B) Q = 10 * 4.18*(373 - 277.22) + 10 * 2260 + 10 * 2.08 * (500 - 373) = 29245 Jouls

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