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Imagine that you have 50 $\mathrm{g}$ of water and 50 $\mathrm{g}$ of methanol, each in a 100 $\mathrm{mL}$ beaker. You place both on a hot plate on low heat.a. Which sample will be at a higher temperature after 5 min? Explain your thinking.b. If the initial temperature of each liquid is $23^{\circ} \mathrm{C},$ what is the temperature of each after 25 cal of energy are transferred from the hot plate to each sample?

a) The methanol will be hotter than water because it has a lower specific heat capacity. methanol does not need to transfer as much thermal energy as aluminum does to raise temperature of some level. So it will be hot sooner.b) $\mathrm{T}=0.5 / 0.58+23=23.86^{\circ} \mathrm{C}$$\mathrm{T}=0.5+23=23.5^{\circ} \mathrm{C}$

Chemistry 102

Chemistry 101

Chapter 18

Observing Energy

Section 5

Specific Heat Capacity

Thermodynamics

Thermochemistry

University of Central Florida

University of Maryland - University College

Brown University

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question. Number eight has a couple parts to it, but the scenario is the same for both parts. We have 50 g, methanol and 50 g of water, both placed into separate beakers. Put on a hot plate. Now we need to make an assumption here before we proceed with Part A. We need to assume that the hotplate is transferring the same amount of heat per unit time to both of them. So after five minutes, methanol would have received the same amount of heat as water would have. We can then look at their specific key capacities. One calorie per gram per degree Celsius and 0.58 calories per gram degrees Celsius. Because methanol has a lower specific heat capacity, then it doesn't need as much heat to have the same change in temperature or if it receives the same amount of heat. It has a greater change in temperature, so methanol is the one that's going to be the warmest After five minutes for Part V. It wants us to calculate the final temperatures for each of them, assuming in the five minutes 25 calories Waas added to both of them. To do that will take. Q is equal to specific heap will do. Water first multiplied by mass multiplied by change in temperature. Final temperature minus initial temperature. The initial temperature was 23. We then get a T final after doing the algebra of 23.5 degrees Celsius. If we do the same thing with methanol having a smaller heat capacity, we should have a higher temperature, which we do of 23.86 or 23.9 degrees Celsius. So is predicted. Methanol with a lower specific heat capacity, has the greatest change in temperature.

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