Let's see, 10.0% of 950 g is 95.0 g. I will first assume that the bricks are starting out at 100°C. So, all you need to do is calculate the heat required to convert 95.0 g of liquid water at 100°C to water vapor at 100°C. The heat of vaporization of water is 2264 J/g. So, we have
95.0 g X 2264 J/g = 215080 J, or 215 kJ. This is answer d.
If the water is starting out at 25°C, then we first have to calculate the heat required to heat it to 100°C. This would be
heat = 95.0 g X 75°C X 4.184 J/g°C = 29811 J, or 29.8 kJ.
The total heat is then 215 kJ + 29.8 kJ = 244.8 kJ.
The problem is not clear about the starting temperature, unfortunately!
If you assume that the initial temperature is 20°C, then you get
heat = 95.0 g X 80°C X 4.184 J/g°C = 31798.4 J, or 31.8 kJ.
Then the total heat is 215 kJ + 31.8 kJ = 246.8 kJ, still not one of the given answers. 
2) First calculate the heat lost by the water:
heat = mass of water X ΔT of the water X specific heat of the water
Then, convert this answer to kJ and divide by the moles of (NH4)2SO4 to get the heat of solution in kJ per mole of (NH4)2SO4 dissolved.
Steve
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