Question

In: Chemistry

At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...

At a particular temperature the equilibrium constant for the reaction:
H2(g) + F2(g) ⇔ 2HF(g)
is K = 64.0. A reaction mixture in a 10.00-L flask contains 0.23 moles each of hydrogen and fluorine gases plus 0.50 moles of HF. What will be the concentration of H2 when this mixture reaches equilibrium?

Solutions

Expert Solution

Equilibrium Quotient expression is
Qc = [HF]^2/[H2]*[F2]
= (0.05^2)/(0.023^1)*(0.023^1)
=4.73

comparing Q and k
since Q is lesser than K
reaction will move in forward direction
ICE Table:

                    [H2]                [F2]                [HF]              


initial             0.023               0.023               0.05              

change              -1x                 -1x                 +2x               

equilibrium         0.023-1x            0.023-1x            0.05+2x           

Equilibrium constant expression is
Kc = [HF]^2/[H2]*[F2]
64.0 = (0.05 + 2*x)^2/(0.023-1*x)^2
sqrt(64.0) = (0.05 + 2*x)/(0.023-1*x)
8.0 = (0.05 + 2*x)/(0.023-1*x)
0.184-8*x = 0.05 + 2*x
0.134-10*x = 0
x = 0.0134

At equilibrium:
[H2] = 0.023-1x = 0.023-1*0.0134 = 0.0096 M

Answer: 0.0096 M

queen_honey_blossom answered 3 years ago
Next > < Previous

Related Solutions

At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is K = 25.0. A reaction mixture in a 10.00-L flask contains 0.33 moles each of hydrogen and fluorine gases plus 0.30 moles of HF. What will be the concentration of H2 when this mixture reaches equilibrium?
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is...
At a particular temperature the equilibrium constant for the reaction: H2(g) + F2(g) ⇔ 2HF(g) is K = 81.0. A reaction mixture in a 10.00-L flask contains 0.25 moles each of hydrogen and fluorine gases plus 0.37 moles of HF. What will be the concentration of H2 when this mixture reaches equilibrium?
Consider the reaction H2 (g) + F2 (g) <-- --> 2HF (g) .At a certain temperature,...
Consider the reaction H2 (g) + F2 (g) <-- --> 2HF (g) .At a certain temperature, 0.50 moles of hydrogen gas, 0.50 moles of fluorine gas and .25 moles of hydrogen fluoride gas are placed in a 5.0 L container. Determine if the gas is at equilibrium or not and predict the direction it will move in order to get to equilibrium. And, for the mixure of the gases, determine the final concentrations of each gas. (use an appropriate table)....
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2...
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g) + I2 (g) ---> 2 HI (g) Kc= 53.3 At this temperature, 0.600 mol of H2 and 0.600 mol of I 2 were placed in a 1.00-L container to react. What concentration of HI is present at equilibrium?
Arrange the following reaction in order of increasing S value. 1. H2(g) + F2(g) 2HF(g) 2....
Arrange the following reaction in order of increasing S value. 1. H2(g) + F2(g) 2HF(g) 2. NH4NO3(s) N2O(g) + 2H2O(I) 3. (NH4)2 Cr2O7(s) Cr2O3(s) + 4H2O(I) +N2(g)
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?
The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g)...
The equilibrium constant (KP) is 0.16 at a particular temperature for the reaction: N2O4(g) ⇌ 2NO2(g) Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur? equilibrium, left, right? PNO2 = 0.154 atm, PN2O4 = 0.148 atm...
The equilibrium constant, K , of a reaction at a particular temperature is determined by the...
The equilibrium constant, K , of a reaction at a particular temperature is determined by the concentrations or pressures of the reactants and products at equilibrium. For a gaseous reaction with the general form aA+bB⇌cC+dD the Kc and Kp expressions are given by Kc=[C]c[D]d[A]a[B]b Kp=(PC)c(PD)d(PA)a(PB)b The subscript c or p indicates whether K is expressed in terms of concentrations or pressures. Equilibrium-constant expressions do not include a term for any pure solids or liquids that may be involved in the...
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
Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture...
Consider the following reaction: H2(g) + I2(g) ⇌ 2HI(g) At a particular temperature, a reaction mixture at equilibrium contains pressures of H2 = 0.958 atm, I2 = 0.877 atm, and HI = 0.020 atm. At the same temperature, a second reaction mixture (not at equilibrium) contains pressures of H2 = 0.621 atm, I2 = 0.621 atm, and HI = 0.101 atm. What will be the partial pressure of HI when the second reaction mixture reaches equilibrium? a) 0.0144 atm b)...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT