Is the first part answer, 0C correct? If so, why is that the answer? I looked online and there's so many different answers for part A. I think 0C should be correct. Thank you so much!

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5. In an insulated vessel, 250 g of ice at 0°C is added to 600 g of water at 18.0°C. (a) What is the final temperature of the system? (b) How much ice remains when the system reaches equilibrium? The latent heat of fusion is 3.33x105 J/kg and the specific heat of water is 4186 J/kg Cº. (a) Since the heat required to melt 250 g of ice at 0°C exceeds the heat required to cool 600 g of water from 18°C to 0°C, the final temperature of the system (water + ice) must be 0°C (b) Let m represent the mass of ice that melts before the system reaches equilibrium at 0°C. cold = -hot mL, -mc (0°C-T) m (3.33x10 J/kg) = -(0.600 kg)(4 186 J/kg-°C) (0°C-18.0°C) m = 136 g, so the ice remaining = 250 g -136 g = 114 g 5. In an insulated vessel, 250 g of ice at 0°C is added to 600 g of water at 18.0°C. (a) What is the final temperature of the system? (b) How much ice remains when the system reaches equilibrium? The latent heat of fusion is 3.33x105 J/kg and the specific heat of water is 4186 J/kg Cº. (a) Since the heat required to melt 250 g of ice at 0°C exceeds the heat required to cool 600 g of water from 18°C to 0°C, the final temperature of the system (water + ice) must be 0°C (b) Let m represent the mass of ice that melts before the system reaches equilibrium at 0°C. cold = -hot mL, -mc (0°C-T) m (3.33x10 J/kg) = -(0.600 kg)(4 186 J/kg-°C) (0°C-18.0°C) m = 136 g, so the ice remaining = 250 g -136 g = 114 g