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Agata [3.3K]
3 years ago
8

If 50 liters of carbon dioxide gas are produced by the reaction below at 273 Kand 100 atm, how oxygen gas were used the reaction

? 2 CO(g) + O2(g) ----> 2 CO2(g)
Chemistry
1 answer:
oee [108]3 years ago
5 0
Using the ideal gas equation:

pV = nRT
n = pV / RT

1atm = 101325Pa, so p = 10132500Pa
1L = 0.001m^3, so V = 0.050m^3
R = 8.214 (ideal gas constant)
T = 273K

Hence moles of CO2 = (10132500 * 0.050) / (8.314 * 273) = 223.2101553

Reaction ratio between oxygen and CO2 is 1:2
Hence moles of O2 = 223... / 2 = 112 moles (3sf)

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Chlorine has two naturally stable isotopes: 35Cl (34.968853 amu) and 37Cl (36.965903 amu). The natural abundance of each isotope
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Answer:

35Cl ⇒ 34.968853 amu  has an abundance of 30.05%

Explanation:

The molar mass of chlorine, (which is the average of all its naturally stable isotope masses), is 36.36575 amu.

There are 2 naturally stable isotopes, this means together they have an abundance of 100%

The isotopes are:

35Cl ⇒ 34.968853 amu  has an abundance of X %

37Cl ⇒ 36.965903 amu  has an abundance of Y %

X + Y = 100%   OR X = 100% - Y

36.36575 = 34.968853X + 36.965903Y  

36.36575 = 34.968853(1-Y) + 36.936.96590365903Y

36.36575 = 34.968853 -34.968853Y + 36.965903Y

1.396897 = 1.99705Y

Y = 0.699 = 69.95%

X = 100-69.9 = 30.05%

To control, we can plug in the following equation:

34.968853 * 0.3005 + 36.965903 * 0.6995 = 36.3658

This means

37Cl ⇒ 36.965903 amu  has an abundance of 69.95 %

35Cl ⇒ 34.968853 amu  has an abundance of 30.05%

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3 years ago
Starting with 1.5052g of BaCl2•2H2O and excessH2SO4, how many grams of BaSO4 can be formed?
muminat
1.5052g BaCl2.2H2O => 1.5052g / 274.25 g/mol = 0.0054884 mol
=> 0.0054884 mol Ba 
<span>This means that at most 0.0054884 mol BaSO4 can form since Ba is the limiting reagent. </span>
<span>0.0054884 mol BaSO4 => 0.0054884 mol * 233.39 g/mol = 1.2809 g BaSO4</span>
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