Question

In: Chemistry

A mixture of 0.02958 mol of O2, 0.01705 mol of NOCl, 0.03162 mol of NO2, and...

A mixture of 0.02958 mol of O2, 0.01705 mol of NOCl, 0.03162 mol of NO2, and 0.008375 mol of Cl2 is placed in a 1.0-L steel pressure vessel at 2458 K.

The following equilibrium is established: 1 O2(g) + 2 NOCl(g) 2 NO2(g) + 1 Cl2(g)

At equilibrium 0.005233 mol of Cl2 is found in the reaction mixture.

(a) Calculate the equilibrium partial pressures of O2, NOCl, NO2, and Cl2.

Peq(O2) = .

Peq(NOCl) = .

Peq(NO2) = .

Peq(Cl2) = .

(b) Calculate KP for this reaction.

KP = .

Solutions

Expert Solution

queen_honey_blossom answered 2 years ago
Next > < Previous

Related Solutions

For the reaction, 2 N2O5--> 4 NO2+O2, the rate of formation of NO2 is 0.004 mol^-1...
For the reaction, 2 N2O5--> 4 NO2+O2, the rate of formation of NO2 is 0.004 mol^-1 s^-1. A) Calculate the rate of disappearance of N2O5 B) Calculate the rate of appearance of O2
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                                   ...
a mixture of 0.2 mol of NO, 0.1 mol of H2 and 0.2 mol of H2O...
a mixture of 0.2 mol of NO, 0.1 mol of H2 and 0.2 mol of H2O is placed in 2.0 L at 300 K. At equal [NO] = 0.062. Calculate K
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O...
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0 L vessel at 300 K. At equilibrium [NO] = 0.062 M. 2 NO(g) + 2H2 ⇌ N2(g) + 2 H2O(g) a. What is the Kc at 300 K? b. What is the Kc of the halved reaction, given, at 300 K? NO(g) + H2 ⇌ ½ N2(g) + H2O(g) c. What is the Kp of part (a) at 300...
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O...
A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: 2NO(g)+2H2(g)←−→N2(g)+2H2O(g) At equilibrium [NO]=0.062M. Calculate the equilibrium concentration of H2. Calculate the equilibrium concentration of N2. Calculate the equilibrium concentration of H2O. Calculate Kc
1. What is the mole fraction of O2 in a mixture of 5.07 g of O2,...
1. What is the mole fraction of O2 in a mixture of 5.07 g of O2, 7.16 g of N2, and 1.33 g of H2? 2. What is the mole fraction of N2 in a mixture of 5.07 g of O2, 7.16 g of N2, and 1.33 g of H2? 3. What is the mole fraction of H2 in a mixture of 5.07 g of O2, 7.16 g of N2, and 1.33 g of H2? 4. What is the partial...
What is the mole fraction of O2 in a mixture of 15.1 g of O2, 8.19...
What is the mole fraction of O2 in a mixture of 15.1 g of O2, 8.19 g of N2, and 2.47 g of H2? 0.237 SubmitPrevious Answers Correct Part B Part complete What is the mole fraction of N2 in a mixture of 15.1 g of O2, 8.19 g of N2, and 2.47 g of H2? 0.147 SubmitPrevious Answers Correct Part C Part complete What is the mole fraction of H2 in a mixture of 15.1 g of O2, 8.19...
A mixture of 0.09581 mol of C2H4, 0.02766 mol of N2, 0.04516 mol of NH3, and...
A mixture of 0.09581 mol of C2H4, 0.02766 mol of N2, 0.04516 mol of NH3, and 0.08098 mol of C6H6 is placed in a 1.0-L steel pressure vessel at 731 K. The following equilibrium is established: 3 C2H4(g) + 1 N2(g) 2 NH3(g) + 1 C6H6(g) At equilibrium 0.006932 mol of N2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of C2H4, N2, NH3, and C6H6. Peq(C2H4) = . Peq(N2) = . Peq(NH3) = . Peq(C6H6)...
A mixture of 0.2063 mol of Cl2, 0.2093 mol of H2O, 0.1887 mol of HCl, and...
A mixture of 0.2063 mol of Cl2, 0.2093 mol of H2O, 0.1887 mol of HCl, and 0.09871 mol of O2 is placed in a 1.0-L steel pressure vessel at 575 K. The following equilibrium is established: 2 Cl2(g) + 2 H2O(g) 4 HCl(g) + 1 O2(g) At equilibrium 0.05821 mol of O2 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of Cl2, H2O, HCl, and O2. (b) Calculate KP for this reaction.
A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and...
A mixture of 0.05263 mol of H2O, 0.01327 mol of CH4, 0.07198 mol of CO, and 0.06917 mol of H2 is placed in a 1.0-L steel pressure vessel at 1303 K. The following equilibrium is established: 1 H2O(g) + 1 CH4(g) 1 CO(g) + 3 H2(g) At equilibrium 0.009871 mol of CH4 is found in the reaction mixture. (a) Calculate the equilibrium partial pressures of H2O, CH4, CO, and H2. Peq(H2O) = . Peq(CH4) = . Peq(CO) = . Peq(H2)...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT