At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) <===> 4C(g) K(c) = 2.93 x 10^(27) If, at this temperature, 2.40 mol of A and 3.70 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium? [A] = ? M [B] = ? M [C] = ? M

Solutions

Expert Solution

3A(g) + 2B(g) <===> 4C(g)

K(c) = 2.93 x 10^(27)

3A(g) + 2B(g) <===> 4C(g)

I 2.4 3.7 0

C -3x -2x 4x

E 2.4-3x 3.7-2x 4x

Kc = [C]^4/[A]^3[B]^2

2.93*10^27 = (4x)^4/(2.4-3x)^3*(3.7-2x)^2

2.93*10^27*(2.4-3x)^3*(3.7-2x)^2 = 256x^4

x = 0.79

[A] = 2.4-3x = 2.4-3*0.79 = 0.03M

[B] = 3.7-2x = 3.7-2*0.79 = 2.12M

[C] = 4x = 4*0.79 = 3.16M

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g)...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant, Kc. 3A(g) + 2B(g) <------> 4C(g) Kc= 3.13x 10^31 If, at this temperature, 1.90 mol of A and 4.00 mol of B are placed in a 1.00-L container, what are the concentrations of A, B, and C at equilibrium?

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A...

At a certain temperature, this reaction establishes an equilibrium with the given equilibrium constant Kc. 3A + 2B -><- 4C kc=1.33x10^27 If at this temperature, 2.00 mol of A and 3.80 mol of B are placed in a 1.00L container, what are the concentrations of A, B, C at equilibrium?

At a certain temperature, the equilibrium constant, Kc, for this reaction is 2.60 SO2(g) + NO2(g)...

At a certain temperature, the equilibrium constant, Kc, for this reaction is 2.60 SO2(g) + NO2(g) <--> SO3(g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 3.12 mol of SO2(g) in order to form 1.30 mol of SO3(g) equilibrium

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature,...

At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. At this temperature, 0.500 mol of H2 and 0.500 mol of I2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?

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.

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌...

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ⇌ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask?

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔...

At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are initially mixed in a 2.0-L flask? At a certain temperature the equilibrium constant, Kc, equals 0.11 for the reaction: 2 ICl(g) ↔ I2(g) + Cl2(g). What is the equilibrium concentration of ICl if 0.45 mol of I2 and 0.45 mol of Cl2 are...

At a certain temperature, the equilibrium constant Kc for this reaction is 53.3 H2 + I2...

At a certain temperature, the equilibrium constant Kc for this reaction is 53.3 H2 + I2 ---> 2HI <--- at this temperature, 0.500 mol of H2 AND 0.500 mol of I2 were placed in 1.00L container to react. What concentration of HI is present at equilibrium? [HI]= ?M

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature,...

At a certain temp, the equilibrium constant for this reaction is 53.3. H2(g)+I2(g)=2HI(g) At this temperature, 0.7 mol of H2 and 0.7 mol of I2 were placed in a 1 L container. What is the concentration of HI present at equilibrium?

For the reaction 3A(g)+3B(g)⇌C(g) Kc = 30.2 at a temperature of 377 ∘C . Calculate the...

For the reaction 3A(g)+3B(g)⇌C(g) Kc = 30.2 at a temperature of 377 ∘C . Calculate the value of Kp. Express your answer numerically. Kp = Part B For the reaction X(g)+3Y(g)⇌3Z(g) Kp = 2.06×10−2 at a temperature of 357 ∘C . Calculate the value of Kc. Express your answer numerically. Kc =

Subjects