If we combine nitrous oxide (NO, laughing gas) with oxygen (O2) we produce nitrogen dioxide (NO2) according to the following reaction:
2NO + O2→ 2NO2
How many grams of NO2 will be produced when 5.00 moles of NO react?
According to the equation, you get five moles NO2, mass=5*(14+32) grams
To determine the grams of NO2 produced when 5.00 moles of NO react, we need to use the stoichiometry of the reaction. Stoichiometry relates the number of moles of reactants and products in a balanced chemical equation.
Here are the steps to calculate the mass of NO2 produced:
Step 1: Balance the chemical equation.
The balanced equation is already provided:
2NO + O2 → 2NO2
Step 2: Determine the molar ratio between NO and NO2.
From the balanced equation, we can see that 2 moles of NO react to produce 2 moles of NO2. This means that the molar ratio between NO and NO2 is 2:2, or simply 1:1.
Step 3: Convert moles of NO to moles of NO2.
Since the molar ratio between NO and NO2 is 1:1, the number of moles of NO2 produced will be equal to the number of moles of NO used. In this case, it is 5.00 moles.
Step 4: Convert moles of NO2 to grams of NO2.
To convert moles of NO2 to grams, we need to use the molar mass of NO2. The molar mass of NO2 is calculated by adding the atomic masses of nitrogen (N) and two oxygen (O) atoms.
- Molar mass of nitrogen (N) = 14.01 g/mol
- Molar mass of oxygen (O) = 16.00 g/mol
Adding these together, we get:
Molar mass of NO2 = 14.01 g/mol + (16.00 g/mol × 2) = 14.01 g/mol + 32.00 g/mol = 46.01 g/mol
Now, using the molar mass of NO2, we can convert the moles of NO2 to grams:
Mass of NO2 = Moles of NO2 × Molar mass of NO2
Mass of NO2 = 5.00 moles × 46.01 g/mol = 230.05 grams
Therefore, when 5.00 moles of NO react, 230.05 grams of NO2 will be produced.