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Montano1993 [528]
3 years ago
11

A sample containing 4.80 g of O2 gas has an initial volume of 15.0 L. What is the final volume, in liters, when each of the foll

owing changes occurs in the quantity of the gas at a constant pressure and temperature?
A. A sample of 0.500 mole of O2 is added to the 4.80 g of O2 in the container.
B. A sample of 2.00 g of O2 is removed.
C. A sample of 4.00 g of O2 is added to the 4.80 g of O2 gas in the container.
Chemistry
1 answer:
neonofarm [45]3 years ago
4 0
The correct answer for the question that is being presented above is this one: "A. A sample of 0.500 mole of O2 is added to the 4.80 g of O2 in the container." A sample containing 4.80 g of O2 gas has an initial volume of 15.0 L. The final volume, in liters, when each of the following changes occurs in the quantity of the gas at a constant pressure and temperature is that <span>A sample of 0.500 mole of O2 is added to the 4.80 g of O2 in the container.</span>
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Explanation:

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<em>∴ n = mass/molar mass = </em>(20 g)/(100.0869 g/mol) <em>= 0.1998 ≅ 0.2 mol.</em>

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Under certain conditions, the equilibrium constant of the reaction below is Kc=1.7×10−3. If the reaction begins with a concentra
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Answer:

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Explanation:

<u>Given:</u>

[SbCl5] = 0 M

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Set-up an ICE table for the given reaction:

               SbCl5(g)\rightleftharpoons SbCl3(g)+Cl2(g)

I                 0                    0.0546     0.0546

C              +x                        -x               -x

E               x                  (0.0546-x)    (0.0546-x)

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= 0.0546-x = 0.0546-0.0457 = 0.0089 M

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