Question

In: Chemistry

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at...

For the reaction: N2(g) + 2 O2(g) ↔ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas?

Solutions

Expert Solution

            N2(g) + 2 O2(g) ↔ 2 NO2(g)

             Kc   = [NO2]^2/[N2][O2]^2

           [O2] = x

           [NO2] = 2x

         Kc   = [NO2]^2/[N2][O2]^2

          8.3*10^-10 = (2x)^2/[N2](x)2

         8.3*10^-10    = 4x^2/[N2]*x^2

       [N2]               = 4/8.3*10^-10   = 4.8*10^9 M

          


Related Solutions

A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2...
A.) For which reaction will Kp = Kc? 2 H2O(l) ↔ 2 H2(g) + O2(g) 2 HgO(s) ↔ Hg(l) + O2(g) S(s) + O2(g) ↔ SO2(g) H2CO3(s) ↔ H2O(l) + CO2(g) CaCO3(s) ↔ CaO(s) + CO2(g) B.) How does an increase in the pressure within the container by the addition of the inert gas E affect the amount of C present at equilibrium for the following reaction? A(g) + 3 B(g) ↔ 2 C(g) + D(g)           ΔH° = -65 kJ...
For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains...
For the reaction: 3H2(g) + N2(g) ↔ 2NH3(g) Kc = 480 At equilibrium, a reaction contains 0.3M N2(g) and 4.0M NH3(g). What is the concentration of H2(g)?
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.055. The reaction...
The reaction N2(g)+O2(g)⇌2NO(g) is carried out at a temperature at which Kc = 0.055. The reaction mixture starts with only the product, [NO] = 0.0200 M, and no reactants. Part A Find the equilibrium concentrations of N2 at equilibrium. Part B Find the equilibrium concentrations of O2 at equilibrium. Part C Find the equilibrium concentrations of NO at equilibrium.
At 200°C, Kc​ = 1.6*10−10 for: N2​O(g) + NO2(g) ⇌ 3 NO(g). If 350 mL of...
At 200°C, Kc​ = 1.6*10−10 for: N2​O(g) + NO2(g) ⇌ 3 NO(g). If 350 mL of NO measured at 797 torr and 25.0°C is placed into a 3.00 L container, what will be the molarity of N2​O at equilibrium when the reaction is heated to 200°C? what is the total equilibrium pressure, in units of torr at 200°C?
The reaction                                     NO(g) + O3 -> NO2(g) + O2(g
The reaction                                     NO(g) + O3 -> NO2(g) + O2(g) was studied in 2 experiments under pseudo-first order conditions. a) [O3] = 1x1014 molecules/cc in excess the [NO] varied as follows   {Note, time is in msec (1 msec = 1x10-3 s)!}             time (msec)                 NO (molecules/cc)                         0                      6x108                           100                  5x108                           500                  2.4x108                         700                  1.7x108                         1000                9.9x107 b) [NO] = 2x1014 molecules/cc in excess                  time (msec)                 O3 (molecules/cc)                         0                      1x1010                         50                    8.4x109                                   ...
at 200 oC Kc = 1.4 x 10-10 for the reaction N2O(g) + NO2(g) <-> 3NO(g)....
at 200 oC Kc = 1.4 x 10-10 for the reaction N2O(g) + NO2(g) <-> 3NO(g). If 300 ml of NO measured at 800 torr and 25 oC is placed in a 4.00 L container. what will be the N2O and NO molar concentrations at equilibrium? What will be the total pressure of the mixture (in torr) at equilibrium at 25 oC? 14.98 Jespersen 7th Ed.
What is the overall order of the reaction below 2 NO(g) + O2(g) → 2 NO2(g)...
What is the overall order of the reaction below 2 NO(g) + O2(g) → 2 NO2(g) if it proceeds via the following rate expression? a) zero-order          b) first-order          c) second-order     d) third-order        e) fourth-order
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP =...
The following reaction N2 (g) + O2 (g) ⇔ 2 NO (g) has a KP = 0.032 at a particular temperature. At that temperature, a vessel is filled with 0.040 atm of N2 (g), 0.040 atm of O2 (g) and 0.043 atm of NO (g). What is the pressure of NO (g) at equilibrium?
The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If...
The value of Kc for the reaction: N2O4(g) ↔ 2NO2 (g) is 0.21 at 373K. If a reaction vessel at that temperature initially contains 0.030M NO2 and 0.030M N2O4, what are the concentrations of the two gases at equilibrium? First, the reaction quotient (Q) [page 645 of textbook] must be calculated, and then use the I.C.E table [page 648-650 of the textbook] to determine the equilibrium concentrations.
At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The initial concentration of...
At 2000 ∘C the equilibrium constant for the reaction 2NO(g)←−→N2(g)+O2(g) is Kc=2.4×103. The initial concentration of NO is 0.250 M . Part A What is the equilibrium concentration of NO? Part B What is the equilibrium concentration of N2? Part C What is the equilibrium concentration of O2? Please show me how to got your results :) Thank you!
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT