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- Aug 13, 2006
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This is probably real simple and I'm makng it harder than it is. If someone can explain it to me like I'm 2, I'd appreciate it because I can't wrap my mind around the explanation in the book:
4NH3 (g) + 7O2 (g) ---> 4NO2 (g) + 6H2O (l)
If 8 moles of NH3 are reacted with 14 moles of O2 in a rigid container with an initial pressure of 11 atm, what is the partial pressure of NO2 in the container when the reaction runs to completion? (assume constant temp)
(A) 4 atm
(B) 6 atm
(C) 11 atm
(D) 12 atm
The answer is A, but I don't get it.
4NH3 (g) + 7O2 (g) ---> 4NO2 (g) + 6H2O (l)
If 8 moles of NH3 are reacted with 14 moles of O2 in a rigid container with an initial pressure of 11 atm, what is the partial pressure of NO2 in the container when the reaction runs to completion? (assume constant temp)
(A) 4 atm
(B) 6 atm
(C) 11 atm
(D) 12 atm
The answer is A, but I don't get it.