Question

tion 19 of 27 > At a certain temperature, a 14.5-L container holds four gases in equilibrium. Their masses are 3.5 g So.. 4.6 g So, 19.7 N,, and 0.98 g N, O. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N20 to form SO3 and NZ? Make sure you balance the reaction using the lowest whole number coefficients. K. = 1

Answer 1

Answer -

Given,

Volume = 14.5 L

Mass of SO₃ = 3.5 g

Mass of SO₂ = 4.6 g

Mass of N₂ = 19.7 g

Mass of N₂O = 0.98 g

Kc = ?

1 SO₂ + 1N₂O $\rightarrow$ 1 SO₃ +1N₂ [Balanced]

So, Kc = [SO₃][N₂]/[SO₂][N₂O] ------------A

We know that,

Molarity = Moles / Volume in L

Also,

Moles = Mass/ Molar Mass

So,

Molarity = Mass / (Molar mass * Volume)

molar mass of SO₃ = 80.066 g/mol

molar mass of SO₂ = 64.066 g/mol

molar mass of N₂ = 28.01 g/mol

molar mass of N₂O =44.01280 g/mol

Put the values in the formula,

Molarity of SO₃ = 3.5 g / (14.5 L * 80.066 g/mol) = 0.003 M

Molarity of SO₂ = 4.6 g / (14.5 L * 64.066 g/mol) = 0.005 M

Molarity of N₂ = 19.7 g / (14.5 L * 28.01 g/mol) = 0.048 M

Molarity of N₂O = 0.98 g / (14.5 L * 44.0128 g/mol) = 0.0015 M

Put these values in A,

Kc = [SO₃][N₂]/[SO₂][N₂O]

Kc = (0.003)(0.048)/(0.005)(0.0015)

Kc = 0.192 [Answer]