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Question
The Ostwald process converts ammonia (NH3) to nitric oxide (NO) by reaction with oxygen in the presence of a catalyst at high temperatures. In a test of the process a reaction vessel is initially charged with 3.90 mol NH3(g) and 4.90 mol O2(g), sealed, and heated at a fixed high temperature. When equilibrium is established the reaction mixture is analyzed and found to contain 2.90 mol NO(g). What is the quantity of NH3(g) in the equilibrium reaction mixture?4NH3(g) + 5O2(g)
4NO(g) + 6H2O(g)A) 1.00 mol NH3(g)
B) 6.80 mol NH3(g)
C) 3.90 mol NH3(g)
D) 1.28 mol NH3(g)
E) 2.00 mol NH3(g)
Answer
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