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Problem: Antimony pentachloride decomposes according to this equation:SbCl5(g) ⇌ SbCl3(g) + Cl2(g)An equilibrium mixture in a 5.00-L flask at 448 °C contains 3.85 g of SbCl  5, 9.14 g of SbCl 3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?

FREE Expert Solution

SbCl5(g) ⇌ SbCl3(g) + Cl2(g)

Calculate the concentration of each at equilibrium:

molar mass SbCl5 = 299.01 g/mol

[SbCl5]=3.85 g SbCl5×1 mol SbCl5299.01 g SbCl55.00 L[SbCl5]=0.01287 mol SbCl55.00 L[SbCl5]=2.575×10-3 mol SbCl5L

[SbCl5] = 2.575x10-3 M


molar mass SbCl3 = 228.11 g/mol

[SbCl3]=9.14 g SbCl3×1 mol SbCl3228.11 g SbCl35.00 L[SbCl3]=0.04007 mol SbCl35.00 L[SbCl3]=8.0137×10-3 mol SbCl3L

[SbCl3] = 8.0137x10-3 M


molar mass Cl2 = 70.9 g/mol

[Cl2]=2.84 g Cl2×1 mol Cl270.9 g Cl25.00 L[Cl2]=0.04006mol Cl25.00 L[Cl2]=8.0113×10-3 mol Cl2L

[Cl2] = 8.0113x10-3 M


Calculate the equilibrium constant, K:

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Problem Details

Antimony pentachloride decomposes according to this equation:
SbCl5(g) ⇌ SbCl3(g) + Cl2(g)
An equilibrium mixture in a 5.00-L flask at 448 °C contains 3.85 g of SbCl  5, 9.14 g of SbCl 3, and 2.84 g of Cl2. How many grams of each will be found if the mixture is transferred into a 2.00-L flask at the same temperature?

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Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.