Question

A sample of water has a mass of 100.0 g. Calculate the amount of heat required to change the sample from ice at -45.0°C to liquid water at 75.0°C. Use the chart to complete the multiple steps required to arrive at the final answer. Type in your answers below using 3 digits.
q1 = ___ kJ
q2 = ___ kJ
q3 = ___ kJ
qtot = ___ kJ

Answer 1

The amount of heat required to change the sample from ice at -45.0°C to liquid water at 75.0°C is 83.8 kJ.

Quantity heat required to convert the ice to liquid

The total quantity of heat required is calculated as follows;

q(tot) = q1(to ice) + q2(fusion of ice) + q3(liquid)

q(tot) = mcΔθ₁  + mΔHf    +   mcΔθ₂

q(tot) = (100)(4.2)(0 - -45) + (334)(100)  + (100)(4.2)(75 - 0)

q(tot) = 18,900 J  +  33,400 J   +  31,500 J

q(tot) = 18.900 kJ  +  33.400 kJ   +  31.500 kJ

q(tot) = 83,800 J = 83.8 kJ

Thus, the amount of heat required to change the sample from ice at -45.0°C to liquid water at 75.0°C is 83.8 kJ.

Learn more about quantity of heat here: brainly.com/question/13439286

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