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Ethylene, $\mathrm{C}_{2} \mathrm{H}_{2},$ a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80$\%$ of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. $\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(l)$ Using the data in the table in Appendix G, calculate $\Delta H^{\circ}$ for the reaction.

Reaction enthalpy is $-88.18 \frac{\mathrm{kJ}}{\mathrm{mol}}$

Chemistry 101

Chapter 5

Thermochemistry

University of Central Florida

Drexel University

Brown University

Lectures

02:29

Chemistry is the science o…

04:42

In chemistry and physics, …

05:54

Ethylene gas, $\mathrm{C}_…

03:27

Ethyl alcohol is prepared …

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Monochloroethane $\left(\m…

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Ethanol, $C_{2} H_{5} OH$,…

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Ethylene $\left(\mathrm{C}…

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Ethane, $\mathrm{C}_{2} \m…

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Ethylene reacts with hydro…

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The reaction of ethane gas…

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Using data in Appendix $4,…

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05:11

Hi there. And welcome to problem number 83. In this problem, we are given a balanced equation. Remember, we have C two h four, just ethylene reacting with water. And it's important to note that both of these are in the gaseous state. He and when these react, they form ethanol, which is in the liquid state. What we're trying to calculate here is the heat of formation. So we need to utilize the appendix to find the values for each of these. Um, the C two h four is 52.4 killer jewels per mole. Okay, the H 20 his negative. 241 0.82 killer jewels per mole. Good. And the ethanol is negative. 2 77 0.6. Killer jewels promote. And again, these air all coming from appendix G. Right? So we are trying to find the heat of formation. Um, we've learned that Hess's law tells us that we can take the heat of formation for the products and subtract those of the reactant since to get the heat of formation for the entire equation. So that is what I'm going to do here to calculate changing and Kalbe. I am going to take the products. The balanced equation tells me there is one mole of Thea Phenol, Okay? And its value is negative to 77.6 killer jewels for every mall. That is the only product in this reaction. So I'm starting with that, and I am going to subtract the reactant. So there is one mole of the C two h four. Okay. And that is 52 4 killer jewels in every mole. Calculate that and add that to the H 20 So again, looking at the balanced equation, there is just one mole of H 20 And it has a value of negative to 41.8 to kill jewels. Permal people. So now we have set up the products and subtracting the reactant from those simplifying a little bit. I find that I have negative 277.6 eligibles minus a negative. 189 0.4 to kill jewels. Of course, two negatives make a positive. So I'm subtracting a negative, which means same result as adding it. He and I get a Delta H to be 88 0.18 And that's gonna be killed. Jewels per mole for this reaction. All right. Thank you so much for watching.

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