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QUESTION
If 15.0 g of H2 reacts with excess N2 according to the following equation what would the pressure of NH3 made be if it were trapped in 2.00 L at 35.0oC: N2 (g) + 3H2 (g) --> 2NH3 (g) (
If 15.0 g of H2 reacts with excess N2 according to the following equation what would the pressure of NH3 made be if it were trapped in 2.00 L at 35.0oC:
N2 (g) + 3H2 (g) --> 2NH3 (g) (GS not EQ thus stoich first and then PV=nRT and the value of
R=0.0821 L*atm/mol*K and 0oC = 273K)
