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5. (CH3) Calculations Using Specific Heat: How many kJ of heat are lost when the body temperature of a patient with 6.0 L blood lowers from 38.6 C to 33.1 C? Hint: Assume the specific heat and density of blood are the same as water. Show your work

Answer :

Final answer:

To calculate the heat lost, use the equation q = mcΔT, where q is the heat lost, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. Calculate the mass of the blood using the density of water. Convert the heat lost from joules to kilojoules.

Explanation:

The amount of heat lost can be calculated using the equation q = mcΔT, where q is the heat lost, m is the mass of the substance, c is the specific heat capacity, and ΔT is the change in temperature.

In this case, since the specific heat and density of blood are assumed to be the same as water, we can use the specific heat capacity of water.

First, calculate the mass of the blood using the density of water: mass = density × volume = 1000 g/L × 6.0 L = 6000 g.

Next, calculate the heat lost using the equation: q = mcΔT = (6000 g) × (4.18 J/g°C) × (38.6°C - 33.1°C) = 1329.72 J.

Finally, convert the heat lost from joules to kilojoules: 1329.72 J ÷ 1000 = 1.33 kJ.

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