Question

How many grams of NO are required to produce 121.0 g of N2 in the following reaction? Show all your work4NH3(8) + 6NO(g) → 5N2(g) + 6H2011).Your Answer:

Answer 1

Step-by-step explanation:

First, let's rewrite the equation here:

4 NH3 + 6 NO -> 5 N2 + 6 H2O.

The equation tells us that 6 moles of NO produces 5 moles of N2.

But the question wants us to find the quantity in grams of NO required if we have 121 g of N2.

1. So first, let's transform 121 g of N2 into moles, using its molar mass (28 g/mol) and the following formula: moles = mass/molar mass

2. Then, we use the equation ratio between NO and N2: 6:5.

3. Then we transform the result into grams of NO, using its molar mass (30.01 g/mol) and the following formula: mass = moles*molar mass

1. moles = 121/28

moles = 4.3 moles of N2

2. 6 moles of NO --- 5 moles of N2

x moles of NO --- 4.3 moles of N2

5x = 4.3*6

x = 25.9/5

x = 5.2 moles of NO

3. mass = 5.2*30.01

mass = 155.6 g

Answer: It will require 155.6 g of NO.