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The heat of vaporization of a liquid $\left(\Delta H_{\mathrm{vap}}\right)$ is the energy required to vaporize $1.00 \mathrm{g}$ of the liquid at its boiling point. In one experiment, $60.0 \mathrm{g}$ of liquid nitrogen (boiling point $-196^{\circ} \mathrm{C}$ ) are poured into a Styrofoam cup containing $2.00 \times 10^{2} \mathrm{g}$ of water at $55.3^{\circ} \mathrm{C} .$ Calculate the molar heat of vaporization of liquid nitrogen if the final temperature of the water is $41.0^{\circ} \mathrm{C}$

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$5.60 \mathrm{kJ} / \mathrm{mol}$

Chemistry 101

Chapter 6

Thermochemistry

Carleton College

Rice University

University of Maryland - University College

Lectures

05:27

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.

06:42

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 for this problem, we're supposed to calculate the molar heat of vaporization of liquid nitrogen, given the experimental set up that we have in the problem. So for the fundamental approach this problem is, we know that the amount of heat that is released from the new liquid nitrogen corresponds to the amount of heat that is absorbed by the water. So we're in. Take advantage of the fact that we know the equation for change in heat, which is that this mass specific heat capacity times change in temperature and we'll do this for the water. So we know that the mass the water 20 grams has given to us in the problem. You know that the specific heat capacity of water with four point waiting for when we confined change in temperature. We know that the final temperature was 41 degrees Celsius and we know that the initial temperature was 55 point. When you plug that all inter calculator, you will get that well, kill Julie heat released, and we can put a negative sign in front of it to signify that you know, we know that this is how much heat is released when we have 60 grams of liquid nitrogen, so that's the proportion that we know. We know that 12 killer jewels of heat are released for every 60 grams of liquid nitrogen that we have, but we want to find the more heat of vaporization, so we need to convert this into moles. So then always to do here is just multiplied by the more mass of liquid nitrogen, which happens to be 28 grams for more. When you put that into calculator, multiple it all out. It's just 5.6 killer jewels promote, and that is the final answer.

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