How many grams of NO are required to produce 145 g of N2 in the following reaction? 4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(l)
a. 155 g
b. 186 g
c. 125 g
d. 145 g
e. 129 g

b. 186 g

Explanation:

Step 1: Write the balanced equation.

4 NH₃(g) + 6 NO(g) → 5 N₂(g) + 6 H₂O(l)

Step 2: Calculate the moles corresponding to 145 g of N₂

The molar mass of nitrogen is 28.01 g/mol.

Step 3: Calculate the moles of NO required to produce 5.18 moles of N₂

The molar ratio of NO to N₂ is 6:5.

Step 4: Calculate the mass corresponding to 6.22 moles of NO

The molar mass of NO is 30.01 g/mol.

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