Mohanty n mous H LI The heat released by the combustion of L of ethanol (molar m

Question

Mohanty n mous H LI The heat released by the combustion of L of ethanol (molar mass 46.1 g/mol) is 5.50 used to heat a,275 kg sample of water that has an initial temperature of 18.00C. What is the final of the water? The specific heat capacity of H20 is 4.184 J Cand the density of ethanol is 0.789 g/mL 2 CH3CH2OH 7O2 (g) 4CO2 (g) 6H20 AHorvn 1368 kJ A. 74.0 °C B. 94.0°C C. 88.4°C E. 56.8°C D. 62.0°C An ideal gas a cylinder was placed in a heater and gained 1.50 J of energy as heat. in If the cylinder increased in volume from 345 mL to 1846 mL ainst an atmospheric pressure of 0.985 atm during this process, what is the change in internal energy of the mai in the cylinder? (1 L atm 101.3 J)

Explanation / Answer

Mass of ethanol , m = density x volume

= 0.789 (g/mL) x 5.50Lx103 (mL/L)

= 4339.5 g

From the balanced equation ,

2 moles = 2x46.1 g of ethanol produces 1368 kJ of heat

4339.5 g of ethanol produces M kJ of heat

M = (4339.5 x 1368) / (2x46.1)

= 64.4x103 kJ

This amount of heat is utilized to heat the water

So Heat utilized , Q = mcdt

Where Q = 64.4x103 kJ

c = specific heat of water = 4.184 J/goC

dt = change in temperature = final - initial

= t - 18.0 oC

m = mass of water = 275 kg = 275x103 g

Plug the values we get t -18.0 = 55.9

t= 73.9 oC

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