1. Nitrogen monoxide is oxidized in air to give brown nitrogen dioxide. Starting with 2.2mol NO, how many moles and how many grams of 02 are required for complete reaction? What mass of NO2,in grams, is produced?

The reaction is

NO+1/2O2 ----> NO2

Then the moles of O2 needed are,

n=2.2*1/2=1.1 mol O2

So the mass is

M=1.1*32=35.2 grams

(Molar mass of O2 is 32 g/mol).

The moles of NO2 produced are,

n=2.2 mol

And the mass,

M=2.2*46=101.2 g

(Molar mass of NO2 is 46 g/mol)

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. 🎪💨

To determine the number of moles of O2 required for the complete reaction, we need to use the balanced chemical equation for the reaction between nitrogen monoxide (NO) and oxygen (O2) to form nitrogen dioxide (NO2):

2 NO + O2 → 2 NO2

From the balanced equation, we can see that it requires 1 mole of O2 to react with 2 moles of NO.

Given that we have 2.2 moles of NO, we can set up a simple proportion to find the number of moles of O2 required:

2 moles NO : 1 mole O2 = 2.2 moles NO : x moles O2

By cross-multiplying and solving for x, we find:

x = (2.2 moles NO) * (1 mole O2 / 2 moles NO) = 1.1 moles O2

So, 1.1 moles of O2 are required for the complete reaction.

To convert this to grams, we need to multiply by the molar mass of O2, which is approximately 32 g/mol:

1.1 moles O2 * 32 g/mol = 35.2 grams O2

Therefore, 35.2 grams of O2 are required for the complete reaction.

Finally, to calculate the mass of NO2 produced, we can use the stoichiometry of the balanced equation. Since the molar ratio between NO and NO2 is 2:2, the number of moles of NO2 produced will be equal to the number of moles of NO consumed.

Thus, the mass of NO2 produced can be obtained by multiplying the number of moles of NO by the molar mass of NO2, which is approximately 46 g/mol:

2.2 moles NO * 46 g/mol = 101.2 grams NO2

Therefore, 101.2 grams of NO2 are produced.

To determine the amount of moles and grams of O2 required for the complete reaction and the mass of NO2 produced, we first need to write a balanced chemical equation for the reaction between nitrogen monoxide (NO) and oxygen (O2).

The balanced chemical equation for the reaction is:
2 NO + O2 → 2 NO2

According to the balanced equation, it takes 1 mole of O2 to react with 2 moles of NO to produce 2 moles of NO2.

1. Determining moles and grams of O2 required:
Given that we have 2.2 moles of NO, we can calculate the moles of O2 required using the mole ratio from the balanced equation.

Since the mole ratio is 1:1 between O2 and NO, we need an equal number of moles of O2 as the moles of NO present.

Therefore, the moles of O2 required for the reaction = 2.2 moles.

To convert the moles of O2 to grams, we need to use the molar mass of O2, which is approximately 32 g/mol.

Molar mass of O2 = 32 g/mol.

Grams of O2 required = Moles of O2 × Molar mass of O2
Grams of O2 required = 2.2 moles × 32 g/mol

2. Determining the mass of NO2 produced:
The balanced equation shows that 2 moles of NO react to form 2 moles of NO2.

Since the mole ratio is 1:1 between NO and NO2, the moles of NO2 formed will be the same as the moles of NO used.

Therefore, the moles of NO2 produced = 2.2 moles.

To convert the moles of NO2 to grams, we need to use the molar mass of NO2, which is approximately 46 g/mol.

Molar mass of NO2 = 46 g/mol.

Mass of NO2 produced = Moles of NO2 × Molar mass of NO2
Mass of NO2 produced = 2.2 moles × 46 g/mol

By calculating the above equations, you will find the required moles and grams of O2, as well as the mass of NO2 produced.