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ioda
3 years ago
8

The molar heat capacity for carbon monoxide at constant volume is CV,m = 20.17 J/(K·mol). A 3.00-L fixed-volume flask contains C

O(g) at a pressure of 8.00 kPa and a temperature of 25.0 °C. Assuming that carbon monoxide acts as an ideal gas and that its heat capacity is constant over the given temperature range, calculate the change in entropy for the gas when it is heated to 800.0 °C.
THIS IS FOR MY HIGHSCHOOL, BUT IS MAINLY COLLEGE STUFF PLEASE HELP ME A BIT ;-;
Chemistry
1 answer:
kompoz [17]3 years ago
5 0

ΔS = 0.250 J·K^(-1)

<em>Step 1</em>. Calculate the <em>moles of CO</em>

From the<em> </em><em>Ideal Gas Law</em>,

<em>n</em> = (<em>pV</em>)/(<em>RT</em>) = (8.00 kPa × 3.00 L)/(8.314 kPa·L·K^(-1)·mol^(-1) × 298.15 K)

= <em>0.009 682 mo</em>l  

Δ<em>S</em> = <em>nC</em>_Vln(<em>T</em>_2/<em>T</em>1)

= 0.0096 82 mol × 20.17 J·K^(-1)mol^(-1) ln(1073.15 K/298.15 K)

=  0.1953 J·K^(-1) × ln3.599 = 0.250 J·K^(-1)

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6 0
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The two effects depends on the nature of a substituent. For instance, species that have a lone pair of electrons often donate electrons by resonance while substituents that are electron deficient take away electrons by resonance.

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8 0
3 years ago
Read 2 more answers
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