/*! 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 4 Imagine that you are climbing a ... [FREE SOLUTION] | 91Ó°ÊÓ

91Ó°ÊÓ

Imagine that you are climbing a mountain. (a) Is the distance you travel to the top a state function? Why or why not? (b) Is the change in elevation between your base camp and the peak a state function? Why or why not? [Section 5.2]

Short Answer

Expert verified
(a) The distance traveled to the top of the mountain is not a state function because it can vary based on the path taken. (b) The change in elevation between the base camp and the peak is a state function because it remains the same regardless of the route taken.

Step by step solution

01

(a) Distance traveled as a state function

In order to determine if the distance traveled to the top of the mountain is a state function, we need to analyze whether the distance depends on the path taken or not. It is crucial to realize that a person could take several different paths up the mountain (direct path, zigzagging, etc.), which could result in different lengths of distance traveled. Since the distance traveled to the top of the mountain can vary based on the path taken, it is not a state function.
02

(b) Change in elevation as a state function

Now we will assess if the change in elevation between the base camp and the peak is a state function. Unlike the distance traveled, the change in elevation is not concerned with the path taken; it is solely concerned with the difference in height between the starting point and the ending point. The change in elevation between the base camp and the peak remains the same regardless of the route taken. Therefore, the change in elevation between the base camp and the peak is a state function.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91Ó°ÊÓ!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Consider the following reaction: $$ \mathrm{CH}_{3} \mathrm{OH}(g) \longrightarrow \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) \quad \Delta H=+90.7 \mathrm{~kJ} $$ (a) Is heat absorbed or released in the course of this reaction? (b) Calculate the amount of heat transferred when \(45.0 \mathrm{~g}\) of \(\mathrm{CH}_{3} \mathrm{OH}(g)\) is decomposed by this reaction at constant pressure. (c) For a given sample of \(\mathrm{CH}_{3} \mathrm{OH}\), the enthalpy change on reaction is \(25.8 \mathrm{~kJ}\). How many grams of hydrogen gas are produced? What is the value of \(\Delta H\) for the reverse of the previous reaction? (d) How many kilojoules of heat are released when \(50.9 \mathrm{~g}\) of \(\mathrm{CO}(g)\) reacts completely with \(\mathrm{H}_{2}(g)\) to form \(\mathrm{CH}_{3} \mathrm{OH}(g)\) at constant pressure?

(a) What is work? (b) How do we determine the amount of work done, given the force associated with the work?

How many grams of methane \(\left[\mathrm{CH}_{4}(g)\right]\) must be combusted to heat \(1.00 \mathrm{~kg}\) of water from \(25.0^{\circ} \mathrm{C}\) to \(90.0^{\circ} \mathrm{C}\), assuming \(\mathrm{H}_{2} \mathrm{O}(l)\) as a product and \(100 \%\) efficiency in heat transfer?

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?

Consider the combustion of liquid methanol, \(\mathrm{CH}_{3} \mathrm{OH}(l)\) : $$ \begin{array}{r} \mathrm{CH}_{3} \mathrm{OH}(l)+\frac{3}{2} \mathrm{O}_{2}(g)-\longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) \\ \Delta H=-726.5 \mathrm{~kJ} \end{array} $$ (a) What is the enthalpy change for the reverse reaction? (b) Balance the forward reaction with whole-number coefficients. What is \(\Delta H\) for the reaction represented by this equation? (c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction? (d) If the reaction were written to produce \(\mathrm{H}_{2} \mathrm{O}(g)\) instead of \(\mathrm{H}_{2} \mathrm{O}(l)\), would you expect the magnitude of \(\Delta H\) to increase, decrease, or stay the same? Explain.

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.