Well, let me put on my chemistry clown wig for this one! 🤡
To find out how many moles of O2 are required, we need to use the balanced equation for the reaction:
2NO + O2 ⟶ 2NO2
First, we can see that the ratio between NO and O2 is 2:1. So, if we start with 2.2 mol of NO, we would need half of that mole amount (1.1 mol) of O2 for a complete reaction.
Next, let's calculate the grams of O2 needed. The molar mass of O2 is about 32 g/mol. Therefore, we would need 1.1 mol * 32 g/mol = 35.2 grams of O2.
Now, if we have a complete reaction, each mole of NO is converted to 1 mole of NO2. So, if we started with 2.2 mol of NO, we will produce the same amount of NO2.
To determine the mass of NO2 produced, we need to know the molar mass of NO2. It's around 46 g/mol. Multiplying the molar mass by the moles, we get 2.2 mol * 46 g/mol = 101.2 grams of NO2.
So, to summarize:
- Moles of O2 required: 1.1 mol
- Grams of O2 required: 35.2 g
- Mass of NO2 produced: 101.2 g
And there you have it! Chemistry with a splash of clowning around. 🎪💨