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Pavel [41]
3 years ago
7

An automobile engine provides 642 Joules of work to push the pistons. In this process the internal energy changes by -2952 Joule

s. Calculate q for the engine. This represents the amount of heat that must be carried away by the cooling system.Calculate the change in the internal energy of the engine.
Chemistry
1 answer:
faust18 [17]3 years ago
4 0

Answer:

Recall from the 1st law of thermodynamic -  Energy Balance gives;

assuming : there is no change in kinetic and potential energy, a steady state process, etc.

ΔU = ΔQ + ΔW

For this system, ΔW = +ve (engine does the work)

ΔU = -2952J

ΔQ = -ve? (Heat energy is been released)

Since the heat energy is removed,  the internal energy must increase by

-2952J = 642J - ΔQ

ΔQ = (642 + 2952) = 3594 J was released from the engine and the amount that must be cooled off

Now to find the change in the internal energy of the engine?

Note that as as soon as the heat is removed, there would not be any change in the internal energy of the system because all the energy from the burning of the measure of fuel has been removed.

so ΔU = 0J

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A strontium hydroxide solution is prepared by dissolving 10.60 gg of Sr(OH)2Sr(OH)2 in water to make 47.00 mLmL of solution.What
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Approximately 1.854\; \rm mol\cdot L^{-1}.

Explanation:

Note that both figures in the question come with four significant figures. Therefore, the answer should also be rounded to four significant figures. Intermediate results should have more significant figures than that.

<h3>Formula mass of strontium hydroxide</h3>

Look up the relative atomic mass of \rm Sr, \rm O, and \rm H on a modern periodic table. Keep at least four significant figures in each of these atomic mass data.

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Calculate the formula mass of \rm Sr(OH)_2:

M\left(\rm Sr(OH)_2\right) = 87.62 + 2\times (15.999 + 1.008) = 121.634\; \rm g \cdot mol^{-1}.

<h3>Number of moles of strontium hydroxide in the solution</h3>

M\left(\rm Sr(OH)_2\right) =121.634\; \rm g \cdot mol^{-1} means that each mole of \rm Sr(OH)_2 formula units have a mass of 121.634\; \rm g.

The question states that there are 10.60\; \rm g of \rm Sr(OH)_2 in this solution.

How many moles of \rm Sr(OH)_2 formula units would that be?

\begin{aligned}n\left(\rm Sr(OH)_2\right) &= \frac{m\left(\rm Sr(OH)_2\right)}{M\left(\rm Sr(OH)_2\right)}\\ &= \frac{10.60\; \rm g}{121.634\; \rm g \cdot mol^{-1}} \approx 8.71467\times 10^{-2}\; \rm mol\end{aligned}.

<h3>Molarity of this strontium hydroxide solution</h3>

There are 8.71467\times 10^{-2}\; \rm mol of \rm Sr(OH)_2 formula units in this 47\; \rm mL solution. Convert the unit of volume to liter:

V = 47\; \rm mL = 0.047\; \rm L.

The molarity of a solution measures its molar concentration. For this solution:

\begin{aligned}c\left(\rm Sr(OH)_2\right) &= \frac{n\left(\rm Sr(OH)_2\right)}{V}\\ &= \frac{8.71467\times 10^{-2}\; \rm mol}{0.047\; \rm L} \approx 1.854\; \rm mol \cdot L^{-1}\end{aligned}.

(Rounded to four significant figures.)

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