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To a sample of water at $23.4^{\circ} \mathrm{C}$ in a constant-pressure calorimeter of negligible heat capacity is added a $12.1$-$\mathrm{g}$ piece of aluminum whose temperature is $81.7^{\circ} \mathrm{C} .$ If the final temperature of water is $24.9^{\circ} \mathrm{C}$ calculate the mass of the water in the calorimeter. (Hint: See Table 6.2.)

$98.56 \mathrm{g}$

Chemistry 101

Chapter 6

Thermochemistry

Carleton College

University of Maryland - University College

Brown University

Lectures

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In chemistry, a chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Both reactants and products are involved in the chemical reactions.

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In chemistry, energy is what is required to bring about a chemical reaction. The total energy of a system is the sum of the potential energy of its constituent particles and the kinetic energy of these particles. Chemical energy, also called bond energy, is the potential energy stored in the chemical bonds of a substance. Chemical energy is released when a bond is broken during chemical reactions.

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So this question asked us to find the mass of water in a container when a piece of aluminum is added and were given some numbers about this entire situation. So the key fundamental thing in solving this problem is the idea that the energy is going to be the energy is going to be conserved and the way we're going to go about solving this problem. This to the fact that the amount of heat that is released by aluminum into the water is equal to the heat that is gained by the water and as a result, the subsequent temperature change in water. So first you want to find the heat change of aluminum, so we're going to use the equation that he is equal to mass time specific heat. Klasky Times the change in temperature So we know that the massive aluminum that was put into this water was 12.1 grams. We also know that the specific eat capacity of aluminum waas 0.0 point 900 Jules Program Senator. The final component, which is a team in temperature, could be calculated from the fact that initially the temperature of the aluminum was 81 0.70 degrees centigrade, and then the final temperature of the water, which includes the aluminum, was 24.9. So then we can multiply that my final minus initial temperature. Now, when you put all of that into your calculator, you'll get that. The answer is negative. 618.55 rules. So, in other words, this number is the change in heat of aluminum. And so we know that in order to conserve the heat in the system or the energy in the system that the heat gained by water must be the exact opposite. This. In other words, Q of H. 20 must have been a positive 618 0.55 jewels. Now we're going to simply were do the exact opposite. Well, we did with aluminum because now we know that 618 0.55 jewels, which is a heat that the water gained, is going to be cool to the math. Really water times the specific heat capacity, water times the change in temperature of the water. So we know that the mass of the water can calculated by simply dividing the heat times the specific heat capacity and the temperature. So what are the specific heat capacity and the change in temperature? Well, the specific heat capacity of water, 4.184 Jules per gram centigrade. And we also know that the changing temperature is a positive 1.5 degree centigrade because it goes from 23.4 initially, and after the aluminum is added and the system comes to an equilibrium, it's 24 points nine. So a additional 1.5 degrees centigrade with those numbers with employed it into the final equation and then the final answer that we get after all of this work is 98 0.56 So that is the total mass of water that was initially in the container, and that's fine.

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