Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

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

Short Answer

Expert verified
(a) Work is the energy transferred to or from an object through the application of force along a displacement. (b) To determine the amount of work done, use the formula \(W = F × d × \cos(\theta)\), where \(W\) represents the work done, \(F\) represents the magnitude of the force applied, \(d\) represents the displacement, and \(\theta\) represents the angle between the force and displacement vectors.

Step by step solution

01

(a) Definition of Work

In physics, work is defined as the energy transferred to or from an object through the application of force along a displacement. In simple words, it represents the energy transferred when a force is applied to an object, and the object moves along the direction of the force.
02

(b) Calculation of Work Done

The amount of work done on an object is calculated using the formula: Work \(W = F × d × \cos(\theta)\) Where: - \(W\) represents the work done, - \(F\) represents the magnitude of the force applied, - \(d\) represents the distance over which the force is applied (displacement), and - \(\theta\) represents the angle between the force vector and the displacement vector. In order to calculate the amount of work done, follow the steps below: 1. Determine the magnitude of the force applied (\(F\)). 2. Determine the distance over which the force is applied (displacement, \(d\)). 3. Determine the angle (\(\theta\)) between the force vector and the displacement vector. 4. Plug the values obtained in steps 1, 2, and 3 into the work done formula and calculate the result. Note that if the force and displacement vectors are in the same direction, the angle \(\theta\) will be 0°, and the \(\cos(0)\) term will be 1, simplifying the work done formula to: Work \(W = F × d\)

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 Vaia!

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

The heat of combustion of fructose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\), is \(-2812 \mathrm{~kJ} / \mathrm{mol}\). If a fresh golden delicious apple weighing \(4.23\) oz \((120 \mathrm{~g})\) contains \(16.0 \mathrm{~g}\) of fructose, what caloric content does the fructose contribute to the apple?

Which will release more heat as it cools from \(50^{\circ} \mathrm{C}\) to \(25^{\circ} \mathrm{C}, 1 \mathrm{~kg}\) of water or \(1 \mathrm{~kg}\) of aluminum? How do you know? [Section 5.5]

From the enthalpies of reaction \(2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g) \quad \Delta H=-483.6 \mathrm{~kJ}\) \(3 \mathrm{O}_{2}(g) \stackrel{-\cdots}{\longrightarrow} 2 \mathrm{O}_{3}(g) \quad \Delta H=+284.6 \mathrm{~kJ}\) calculate the heat of the reaction $$ 3 \mathrm{H}_{2}(g)+\mathrm{O}_{3}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(g) $$

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?

Burning methane in oxygen can produce three different carbon-containing products: soot (very fine particles of graphite), \(\mathrm{CO}(\mathrm{g})\), and \(\mathrm{CO}_{2}(\mathrm{~g})\). (a) Write three balanced equations for the reaction of methane gas with oxygen to produce these three products. In each case assume that \(\mathrm{H}_{2} \mathrm{O}(l)\) is the only other product. (b) Determine the standard enthalpies for the reactions in part (a). (c) Why, when the oxygen supply is adequate, is \(\mathrm{CO}_{2}(g)\) the predominant carbon- containing product of the combustion of methane?

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.

Sign-up for free