1. 2O3(g)↔ 3O2(g) ; if 10.0g of O2 is at equilibrium with 7.50g of O3 calculate Kp if the total pressure is 1.10atm.
A. 2.94
B. 0.499
C. 0.339
^ I submitted this question already but the answer was wrong, I worked through it and still couldn't find one of these options. Suggestions?
2. For: N2(g) + O2(g) ↔ 2NO(g) 0.500M O2 and 0.750M N2 is allowed to reach equilibrium. Kc = 1.00 x 10-1. Calculate equilibrium concentration of N2
A. 0.667
B. 0.167
C. 0.083
*Hint from professor: Are the given concentrations equilibrium concentrations or initial? Please read carefully.* Please show how to set up given the hint.
1.
The molar masses of O2 and O3 are 32 g/mol and 48 g/mol
respectively.
The number of moles are obtained by dividing mass with molar
mass.
The number of moles of
The number of moles of
The mole fraction of O2
The mole fraction of O3 = 1- 0.667 = 0.334
The partial pressure of O2
atm
The partial pressure of O3
atm
Hence, the option (A) is the answer.
1. 2O3(g)↔ 3O2(g) ; if 10.0g of O2 is at equilibrium with 7.50g of O3 calculate...
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