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Serggg [28]
3 years ago
5

According to the ideal gas law, a 9.585 mol sample of krypton gas in a 0.8032 L container at 504.9 K should exert a pressure of

494.4 atm. What is the percent difference between the pressure calculated using the van der Waals' equation and the ideal pressure? For Kr gas, a = 2.318 L2atm/mol2 and b = 3.978×10-2 L/mol. %
Chemistry
1 answer:
natka813 [3]3 years ago
6 0

Answer:

1.17%

Explanation:

The pressure using vander waals' equation = 610.955atm

The difference

  • 610.955-494.4 =116.555atm

The % difference = 1.17%

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Calculate δ h for the reaction:no (g) + o2 (g) ↔ no2 (g). given: 2o3(g) ↔ 3o2(g) δh=-426 kj o2(g) ↔ 2o(g) δh=+ 490 kj no(g) + o3
maks197457 [2]
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</span>O3 -----> 1.5O2    δ h = -213  kj             eq. (4)

Then, we subtract eq. (3) by eq. (4) 

NO + O3 ----->  NO2 + O2   δ h = -200 kj
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eq. (2) divided by -2. (Note: Dividing or multiplying by negative number reverses the reaction)

O -----> 0.5O2  <span>δ h = -245  kj         eq. (6)
</span>
Add eq. (6) to eq. (5), we get

NO -----> NO2 - 0.5O2        δ h = 13  kj 
+  O -----> 0.5O2                 δ h = -245  kj
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<em>ANSWER:</em> <em>NO + O ----> NO2               δ h = -232 kj</em>


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