/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 33 You are given \(\Delta H\) for a... [FREE SOLUTION] | 91影视

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Chapter 5: Problem 33

You are given \(\Delta H\) for a process that occurs at constant pressure. What additional information do you need to determine \(\Delta E\) for the process?

Short Answer

Expert verified
To determine the change in internal energy (螖E) for a process occurring at constant pressure, given the enthalpy change (螖H), we need to know the constant pressure (P) and the change in volume (螖V) for the process. We can then use the relationship \(螖H = 螖E + P螖V\) to calculate 螖E.

Step by step solution

01

Understand the relationship between 螖H, 螖E, pressure, and volume

For a process at constant pressure, we can use the relationship between enthalpy change (螖H) and internal energy change (螖E) to find 螖E. The relationship is given by the following formula: \[螖H = 螖E + P螖V\] Here, P is the constant pressure, and 螖V is the change in volume.
02

Identify the required additional information

To determine 螖E, we will need to know the values of the following parameters: 1. The constant pressure (P) of the process 2. The change in volume (螖V) during the process Since we already have been given 螖H, we only lack these two parameters to calculate 螖E using the formula mentioned in Step 1.
03

Conclusion

In order to determine the change in internal energy (螖E) for a process occurring at constant pressure, given the enthalpy change (螖H), we need to know the constant pressure (P) and the change in volume (螖V) for the process.

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Most popular questions from this chapter

Consider the following unbalanced oxidation-reduction reactions in aqueous solution: $$ \begin{aligned} \mathrm{Ag}^{+}(a q)+\mathrm{Li}(s) & \longrightarrow \mathrm{Ag}(s)+\mathrm{Li}^{+}(a q) \\ \mathrm{Fe}(s)+\mathrm{Na}^{+}(a q) & \longrightarrow \mathrm{Fe}^{2+}(a q)+\mathrm{Na}(s) \\ \mathrm{K}(s)+\mathrm{H}_{2} \mathrm{O}(l) & \longrightarrow \mathrm{KOH}(a q)+\mathrm{H}_{2}(g) \end{aligned} $$ (a) Balance each of the reactions. (b) By using data in Appendix C, calculate \(\Delta H^{\circ}\) for each of the reactions. (c) Based on the values you obtain for \(\Delta H^{\circ}\), which of the reactions would you expect to be thermodynamically favored? (That is, which would you expect to be spontaneous?) (d) Use the activity series to predict which of these reactions should occur. ono (Section 4.4) Are these results in accord with your conclusion in part (c) of this problem?

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