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How much energy is required to raise the temperature of 50 g of methanol from $20^{\circ} \mathrm{C}$ to $70^{\circ} \mathrm{C} ?$

1450 $\mathrm{cal}$

Chemistry 102

Chemistry 101

Chapter 18

Observing Energy

Section 5

Specific Heat Capacity

Thermodynamics

Thermochemistry

University of Central Florida

Drexel University

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to answer. Question number six. We simply need to know the heat equation que will be equal to the specific heat of the substance multiplied by the mass of the substance multiplied by the change in temperature. And the change in temperature is T final minus T initial. So if we have something like methanol, then we can go to the table on Page 501 and look at the specific heat of methanol, and we see that the specific heat of methanol is not there. But if we look at the problem just below it, they use the specific heat of methanol as 0.58 calories per gram degrees Celsius. So that's what we'll use, and you'll notice that it is very similar to a compound that is also similar to methanol. Ethanol 0.57 But we'll use 0.58 so we have que then being equal to the mass of methanol. Well specific heat of methanol. Zero point 58 calories program degree Celsius multiplied by its mass 50 g multiplied by its change in temperature. Final temperature. 70 degrees Celsius. Minus initial temperature. 20 degrees Celsius. This gives us the heat value of 1450 calories

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