Question

Consider the reaction of nitric oxide (NO) and oxygen yielding nitrogen dioxide: 2 NO + 02 —> 2 N02 Assume you start with 3.5 mol of NO. How many moles of 02 do you need for the reaction to go to completion? How many grams of N02 will the reaction produce? 0 3.5 mol of 02; 110 g of N02 O 1.8 mol of 02; 110 g of N02 0 1.8 mol of 02; 160 g of N02 O 3.5 mol of 02; 160 g of N02 O 1.8 mol of 02; 140 g of N02

Answer 1

The correct answer is:

1.8 mol of O2; 161 g of NO2.

Step-by-step explanation:

To determine the stoichiometry of the reaction and the amounts of substances involved, we can use the balanced chemical equation:

2 NO + O2 → 2 NO2

From the balanced equation, we can see that for every 2 moles of NO, we need 1 mole of O2 to react and produce 2 moles of NO2.

Given that we start with 3.5 mol of NO, we can calculate the required amount of O2:

2 moles of NO require 1 mole of O2

3.5 moles of NO require (1/2) × 3.5 = 1.75 moles of O2

Therefore, we need 1.75 moles of O2 for the reaction to go to completion.

Now, let's calculate the mass of NO2 produced using the stoichiometry of the reaction:

From the balanced equation, we know that 2 moles of NO react to produce 2 moles of NO2. Therefore, the molar ratio between NO and NO2 is 1:1.

Given that we start with 3.5 mol of NO, we can conclude that 3.5 mol of NO2 will be produced.

To calculate the mass of NO2, we need to know its molar mass, which is 46 g/mol.

Mass of NO2 = Number of moles × Molar mass

Mass of NO2 = 3.5 mol × 46 g/mol = 161 g

Therefore, the reaction will require 1.75 mol of O2 and produce 161 g of NO2.

The correct answer is:

1.8 mol of O2; 161 g of NO2.