Ammonia burns in oxygen as `2NH_(3)(g)+2.5O_(2)(g) to 2NO(g)+3H_(2)O(g)`
What mass of steam is produced when 1.5 g NO is formed?

Explanation

To solve the problem of finding the mass of steam produced when 1.5 g of NO is formed from the reaction of ammonia with oxygen, we can follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ 2NH_3(g) + 2.5O_2(g) \rightarrow 2NO(g) + 3H_2O(g) \]

### Step 2: Calculate the molar mass of NO
To find the molar mass of NO (Nitric Oxide):
- Molar mass of Nitrogen (N) = 14 g/mol
- Molar mass of Oxygen (O) = 16 g/mol
- Therefore, molar mass of NO = 14 + 16 = 30 g/mol

### Step 3: Determine the mass of steam produced from the stoichiometry of the reaction
From the balanced equation, we see that 2 moles of NO produce 3 moles of H2O (steam).

- Molar mass of H2O (Water):
- Molar mass of Hydrogen (H) = 1 g/mol
- Therefore, molar mass of H2O = (2 × 1) + 16 = 18 g/mol
- For 2 moles of NO (60 g), the mass of steam produced is:
- 3 moles of H2O = 3 × 18 g = 54 g

### Step 4: Set up a proportion to find the mass of steam produced from 1.5 g of NO
Using the relationship from the balanced equation:
- If 60 g of NO produces 54 g of H2O,
- Then 1.5 g of NO will produce:
\[ \text{Mass of steam} = \left(\frac{54 \text{ g H2O}}{60 \text{ g NO}}\right) \times 1.5 \text{ g NO} \]

### Step 5: Calculate the mass of steam produced
\[ \text{Mass of steam} = \left(\frac{54}{60}\right) \times 1.5 = 1.35 \text{ g} \]

### Final Answer
The mass of steam produced when 1.5 g of NO is formed is **1.35 g**.

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