A student fills two identical beakers with the sane volumeof water.The student places one beaker in a freezerand the other beake
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The question is incomplete, here is the complete question:
A reaction
has a standard free-energy change of -4.88 kJ/mol at 25°C
What are the concentrations of A, B, and C at equilibrium if at the beginning of the reaction their concentrations are 0.30 M, 0.40 M and 0 M respectively?
<u>Answer:</u> The equilibrium concentrations of A, B and C are 0.117 M, 0.217 M, 0.183 M respectively.
<u>Explanation:</u>
Relation between standard Gibbs free energy and equilibrium constant follows:
where,
= Standard Gibbs free energy = -4.88 kJ/mol = -4880 J/mol (Conversion factor: 1 kJ = 1000 J)
R = Gas constant =
T = temperature =
= equilibrium constant of the reaction
Putting values in above equation, we get:
We are given:
Initial concentration of A = 0.30 M
Initial concentration of B = 0.40 M
Initial concentration of C = 0 M
The chemical reaction follows:
<u>Initial:</u> 0.30 0.40 0
<u>At eqllm:</u> 0.30-x 0.40-x x
The expression of equilibrium constant for the above reaction follows:
We are given:
Putting values in above equation, we get:
Neglecting the value of x = 0.657, because change cannot be greater than the initial concentration
So, equilibrium concentration of A =
Equilibrium concentration of B =
Equilibrium concentration of C =
Hence, the equilibrium concentrations of A, B and C are 0.117 M, 0.217 M, 0.183 M respectively.
Hey mate here is pratyush for your help from India
..
your answer is in the attachment ..
the answer is 68g of NH3 will be produced.
hope it helps you.
be brainly
..
your answer is in the attachment ..
the answer is 68g of NH3 will be produced.
hope it helps you.
be brainly