Question
In: Chemistry
The equilibrium constant KC for the reaction below has a value of 2.80 x 10^2 at...
The equilibrium constant KC for the reaction below has a value of 2.80 x 10^2 at a certain temperature. Suppose that for a particular system at equilibrium at that certain temperature the SO2 molar density is 0.0124 mol/L and the O2 molar density is 0.0310. Please predict the molar density of SO3.
2SO2 (g) + O2 (g) →2SO3 (g)
Solutions
Expert Solution
Let we have a equilibrium reaction as
then the equilibrium constant 
of the above
equilibrium reaction is written as
Here the Equilibrium reaction is written as
As we know that of the above
equilibrium reaction is written as
We have the given concentration as
Now by using the law
Hence the concentration of 
at
equilibrium is found as 0.0362M.
queen_honey_blossom answered 2 years agoRelated Solutions
The equilibrium constant, K, for the reaction shown below has a value 1.8 x 105. In...
The equilibrium constant, K, for the reaction shown
below has a value 1.8 x 105. In this reaction which is the
strongest acid and which is the strongest base?
CH3CO2H(aq) + H2O (l) --->H3O+(aq) + CH3CO2-(aq)
please explain why?
a) Give the mathematical equilibrium constant expression Kc and Kp (not the value!) for the reaction...
a) Give the mathematical equilibrium constant expression Kc and
Kp (not the value!) for the reaction
2N2O5(g) ↔ 4NO2 (g) + O2(g)
b) At 250oC the concentrations of N2O5, NO2 and O2 are 0.100
mol/L, 0.0283 mol/L and 0.0105 mol/L. Calculate the values for Kc
and Kp
. The equilibrium constant for the reaction below is 7.796 x 10-9. Calculate the equilibrium concentrations...
. The equilibrium constant for the reaction below is 7.796 x
10-9. Calculate the equilibrium concentrations of all
species if the initial Co3+ concentration is 0.425 M and
the initial SO42- concentration is 0.113
M.
2 Co3+(aq) + 2
SO42-(aq)→←
2 Co2+(aq) +
S2O82-(aq)
Find the value of the equilibrium constant Kc at 460°C for the reaction- ½ H2(g) +...
Find the value of the equilibrium constant Kc at 460°C for the
reaction-
½ H2(g) + ½ I2(g)
HI(g)
given the following data: A 4.50-mol sample of HI is placed in a
1.00-L vessel at 460°C, and the reaction system is allowed to come
to equilibrium. The HI partially decomposes, forming 0.343 mol H2
at equilibrium.
A) 0.0123 B) 0.0081 C) 0.0309 D) 11.1 E) 5.69
The equilibrium constant Kc for the reaction below is 0.00427 at a certain temperature. Br2(g) ⇌...
The equilibrium constant Kc for the reaction below is 0.00427 at
a certain temperature. Br2(g) ⇌ 2Br(g) If the initial
concentrations are [Br2] = 0.0844 M and [Br] = 0.0763 M, calculate
the concentrations of these species at equilibrium.
1) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) <---...
1) The equilibrium constant, Kc, for the following reaction is
1.20×10-2 at 500 K. PCl5(g) <--- --->PCl3(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.279 moles of PCl5(g) are introduced into a 1.00 L vessel at
500 K. [PCl5] = M [PCl3] = M [Cl2] = M 2) The equilibrium constant,
Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)
<---- ----> 2 HI (g) Calculate the equilibrium concentrations
of...
1) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) <---...
1) The equilibrium constant, Kc, for the following reaction is
1.20×10-2 at 500 K. PCl5(g) <--- --->PCl3(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.279 moles of PCl5(g) are introduced into a 1.00 L vessel at
500 K. [PCl5] = M [PCl3] = M [Cl2] = M 2) The equilibrium constant,
Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)
<---- ----> 2 HI (g) Calculate the equilibrium concentrations
of...
The equilibrium constant Kc for the reaction N2O4 <—> 2 NO2 at 25degrees C is 170....
The
equilibrium constant Kc for the reaction
N2O4 <—> 2 NO2 at 25degrees C is 170. Suppose 13.3g of
N2O4 is placed in a 4.000-L flask at 25 C.
Calculate the percentage of the original N2O4 that is
dissociated?
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following
reaction is 4.10 × 10–4.
N2 (g) +O2 (g) <---> 2NO (g)
What percentage of O2 will react to form NO if 0.737 mol of N2
and 0.737 mol of O2 are added to a 0.645-L container and allowed to
come to equilbrium at 1700 °C?
At 1700 °C, the equilibrium constant, Kc, for the following reaction is 4.10 × 10–4. N2...
At 1700 °C, the equilibrium constant, Kc, for the following
reaction is 4.10 × 10–4.
N2 (g) +O2 (g) <---> 2NO (g)
What percentage of O2 will react to form NO if 0.737 mol of N2
and 0.737 mol of O2 are added to a 0.645-L container and allowed to
come to equilbrium at 1700 °C?
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