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
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]
tion 19 of 27 > At a certain temperature, a 14.5-L container holds four gases in...
At a certain temperature, a
24.5-L container holds four gases in equilibrium. Their masses are
3.5 g SO3 , 4.6 g SO2 , 13.4 g N2 , and 0.98 g N2O .
SO,, 13.4 g 52T At a certain temperature, a 24.5-L container holds four gases in equilibrium. Their masses are 3.5 g SO2,4 Ny, 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...
At a certain temperature, a 27.0-L container holds four gases in equilibrium. Their masses are 3.5 g So,, 4.6 g So,. 15.7 g N and 0.98 g N, O. What is the value of the equilibrium constant at this temperature for the reaction of So, with N20 to form SO3 and Nz? Make sure you balance the reaction using the lowest whole number coefficients. K-
At a certain temperature, a 19.0-L container holds four gases in equilibrium. Their masses are 3.5 g SO2, 4.6 g SO,, 25.0 g Ny, 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 N2? Make sure you balance the reaction using the lowest whole-number coefficients. Kc = 64.5
At a certain temperature, a 17.5-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3. 4.6 g SO2, 23.0 g N2, and 0.98 g N20. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N20 to form and N2 (balanced with lowest whole-number coefficients)? Number
At a certain temperature, a 17.5-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3. 4.6 g SO2, 23.0 g N2,...
At a certain temperature, a 10.5-L container holds four gases in equilibrium. Their masses are 3.5 g SO,, 4.6 g So, 14.3 g N., and 0.98 g N.o. What is the value of the equilibrium constant at this temperature for the reaction of SO, with N20 to form SO3 and N2? Make sure you balance the reaction using the lowest whole number coefficients. K = 0.65691
At a certain temperature, a 11.5 -L container holds four gases in equilibrium. Their masses are 3.5 g SO 3 , 4.6 g SO 2 , 18.8 g N 2 , and 0.98 g N 2 O . What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2? Make sure you balance the reaction using the lowest whole-number coefficients. Kc=
stion 10 of 15 > At a certain temperature, a 14.5-L container holds four gases in equilibrium. Their masses are 3.5 g Sog, 4.6 g SO2, 19.2 g N,, and 0.98 g N,0. What is the value of the equilibrium constant at this temperature for the reaction of So, with N20 to form So; and N2? Make sure you balance the reaction using the lowest whole-number coefficients. K = At a certain temperature, 0.780 mol SO, is placed in a...
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At a certain temperature, a 20.5-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3, 4.6 g SO2, 21.5 g N2, and 0.98 g N2O. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2 (balanced with lowest whole-number coefficients)?