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Calculate \(\Delta E\) for each of the following. a. \(q=-47 \mathrm{kJ}, w=+88 \mathrm{kJ}\) b. \(q=+82 \mathrm{kJ}, w=-47 \mathrm{kJ}\) c. \(q=+47 \mathrm{kJ}, w=0\) d. In which of these cases do the surroundings do work on the system?

Short Answer

Expert verified
The calculated values for \(\Delta E\) are: a. \(\Delta E = 41 \mathrm{kJ}\) b. \(\Delta E = 35 \mathrm{kJ}\) c. \(\Delta E = 47 \mathrm{kJ}\) The surroundings do work on the system in case a.

Step by step solution

01

Case a: \(q=-47 \mathrm{kJ}, w=+88 \mathrm{kJ}\)

Given \(q = -47 \mathrm{kJ}\) and \(w = 88 \mathrm{kJ}\), we can calculate \(\Delta E\) using the formula: \[\Delta E = q + w = -47 + 88\] Now solve for \(\Delta E\): \[\Delta E = 41 \mathrm{kJ}\]
02

Case b: \(q=+82 \mathrm{kJ}, w=-47 \mathrm{kJ}\)

Given \(q = 82 \mathrm{kJ}\) and \(w = -47 \mathrm{kJ}\), we can calculate \(\Delta E\) using the formula: \[\Delta E = q + w = 82 - 47\] Now solve for \(\Delta E\): \[\Delta E = 35 \mathrm{kJ}\]
03

Case c: \(q=+47 \mathrm{kJ}, w=0\)

Given \(q = 47 \mathrm{kJ}\) and \(w = 0\), we can calculate \(\Delta E\) using the formula: \[\Delta E = q + w = 47 + 0\] Now solve for \(\Delta E\): \[\Delta E = 47 \mathrm{kJ}\]
04

Identifying cases where surroundings do work on the system

To determine in which cases the surroundings do work on the system, we need to analyze the sign of the \(w\) values. If \(w\) is positive, that means the surroundings are doing work on the system, and if \(w\) is negative, the system is doing work on the surroundings. - Case a: \(w = +88 \mathrm{kJ}\), surroundings do work on the system. - Case b: \(w = -47 \mathrm{kJ}\), system does work on the surroundings. - Case c: \(w = 0\), no work is done. So, in case a, the surroundings do work on the system.

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Most popular questions from this chapter

The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area \((1 \text { watt }=1 \mathrm{Js} \text { ). The plants in an }\) agricultural field produce the equivalent of \(20 . \mathrm{kg}\) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right)\) per hour per hectare \(\left(1 \mathrm{ha}=10,000 \mathrm{m}^{2}\right) .\) Assuming that sucrose is produced by the reaction $$ \begin{aligned} 12 \mathrm{CO}_{2}(g)+11 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}(s)+& 12 \mathrm{O}_{2}(g) \\ & \Delta H=5640 \mathrm{kJ} \end{aligned} $$ calculate the percentage of sunlight used to produce the sucrose-that is, determine the efficiency of photosynthesis.

Explain why \(\Delta H\) is obtained directly from coffee-cup calorimeters, whereas \(\Delta E\) is obtained directly from bomb calorimeters.

Consider the following equations: $$ \begin{array}{ll}{3 \mathrm{A}+6 \mathrm{B} \longrightarrow 3 \mathrm{D}} & {\Delta H=-403 \mathrm{kJ} / \mathrm{mol}} \\ {\mathrm{E}+2 \mathrm{F} \longrightarrow \mathrm{A}} & {\Delta H=-105.2 \mathrm{kJ} / \mathrm{mol}} \\\ {\mathrm{C} \longrightarrow \mathrm{E}+3 \mathrm{D}} & {\Delta H=64.8 \mathrm{kJ} / \mathrm{mol}}\end{array} $$ Suppose the first equation is reversed and multiplied by \(\frac{1}{6},\) the second and third equations are divided by \(2,\) and the three adjusted equations are added. What is the net reaction and what is the overall heat of this reaction?

What is incomplete combustion of fossil fuels? Why can this be a problem?

In a coffee-cup calorimeter, 50.0 \(\mathrm{mL}\) of 0.100\(M \mathrm{AgNO}_{3}\) and 50.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M} \mathrm{HCl}\) are mixed to yield the following reaction: $$\mathrm{Ag}^{+}(a q)+\mathrm{Cl}^{-}(a q) \longrightarrow \mathrm{AgCl}(s)$$ The two solutions were initially at \(22.60^{\circ} \mathrm{C}\) , and the final temperature is \(23.40^{\circ} \mathrm{C}\) Calculate the heat that accompanies this reacture in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 100.0 \(\mathrm{g}\) and a specific heat capacity of 4.18 \(\mathrm{J} / \rho \mathrm{C} \cdot \mathrm{g} .\)

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