Consider the reaction:
2 NO(g) + 5 H2(g)-2 NH3(g) + 2 H2O(g)
A reaction mixture initially contains 5 moles of NO and 10 moles of H2. Without doing any calculations, determine which set of amounts best represents the mixture after the reactants have reacted as completely as possible. Explain your reasoning.
a. 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O
b. 0 mol NO, 1 mol H2, 5 mol NH3, 5 mol H2O
c. 3 mol NO, 5 mol H2, 2 mol NH3, 2 mol H2O
d. 0 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O

After the whole feasible response of balanced equation, 1 mole of NO has remained withinside the response mixture is 1 mol NO, 0 mol H2, 4 mol NH3, 4 mol H2O.

The balanced chemical equation for

the response will be: 2 NO(g) + 5 H2(g)-2 NH3(g) + 2 H2O(g). The hydrogen required has been:

2 moles NO = 5 moles hydrogen
five moles NO Hydrogen five 2 G x 5 moles
five moles NO = 5 moles Hydrogen.
The to be had hydrogen has been 10
moles.
5 moles hydrogen = 2 moles NO
2 10 moles hydrogen NO x 10 moles
10 moles hydrogen = four moles NO.
The whole usage of hydrogen calls for four moles of NO. The to be had NO has been 5 moles. The final NO has been given as:
Remaining NO = Total - consumed
Remaining NO = 5-4
Remaining NO = 1mole
After the whole feasible response of the mixture, 1 mole of NO has remained withinside the response mixture.

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