0.2 mole of A and 0.4 mile of B were reacted at a certain temperature and allowed to come to equilibrium . A+B---2AB The equilibrium mixture contained 0.1 mole of A, find Kc if volume of the container was 2 dm^3?

Answer 1

#color(red)(K_c = 13.4)#

I'll show my explanation in steps for your understanding

  1. First set balance the equation
#2A + 2B = 2AB#
  1. Now write the equilibrium constant for the reaction
#color(blue)(K_c = ([AB])/([A] [B]))#
3. As #color(blue)(K_c)# is being determined the temperature matters and thus volume also matters.So the conversion of moles to molarity is necessary
#M = "moles"/L#
4. As the volume of the container is #"2dm"^3#
Conversionof #dm^3# to litres is necessary
#1dm^3 = 1L#
#therefore# #2dm^3 = 2L#
  1. Calculate the molarities
Conc. of A = #"0.2moles"/(2L) = 0.1M#
Conc. of B = #"0.4mole"/(2L) = 0.2M#
Conc. of A at equilibrium #"0.1moles"/(2L) = 0.05M#
  1. Set up an ICE table
#color(blue)("For problems related to equilibrium") # #color(blue) ("concentrations,you need to set up an ICE table.")#
#color(white)(mmmmml)"2A" color(white)(lm)+ color(white)(mmmm)"2B"color(white)(llll) → color(white)(ml) 2AB# #"I/mol:"color(white)(mll)0.1Mcolor(white)(mmmmml)0.2Mcolor(white)(mmmmml)0# #"C/mol:"color(white)(m)-xcolor(white)(mmmmmm)-xcolor(white)(mmmm)+2x# #"E/mol:"color(white)(lm)0.1M-xcolor(white)(mml)0.2M-xcolor(white)(lmmml)2x#
From the given information we know that the equilibrium amount of A is 0.05M. Thus #0.1M - x = 0.05M#
Solve for #x#
#0.1M - x = 0.05M# #x = 0.1M-0.05M# #x = 0.05M#
  1. Solve for the equilibrium amounts of B and AB
#AB = 2x = 2 xx 0.05M = 0.1M# #B = 0.2M - 0.05M = 0.15M# And we know the equilibrium amounts of A
7. Now solve for #K_c#
#K_c = "products"/"reactants"#
#K_c = ([ 0.1M])/([0.05M][0.15M])#
#K_c =13.333#
If you want #color(blue)("three sig figs")#
#K_c = 13.4#
You can also calculate the #Q_c# to see to which direction will the reaction proceed
#color(blue)(Q_c = ([AB]^2)/([A]^2[B]^2))#
#Q_c = 177.777777778#
As #color(purple)(K_c < Q_c) #

Reaction will proceed towards left

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Answer 2

Kc = [AB]² / [A][B] Kc = (0.1 mol / 2 dm³)² / [(0.2 mol - 0.1 mol) / 2 dm³][(0.4 mol - 0.1 mol) / 2 dm³]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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