3 NO2(g) + H2O(l)--->2 HNO3(aq) + NO(g)
Suppose someone needs 25.0 kg of HNO3. How much NO2 should they start with to end up with the amount they need?
25kg of HNO3? How many moles of HNO3 is that...figure it. Then, the mole ratio tells that you want 3/2 (1.5 x) as many moles of NO2, convert that to grams.
To determine the amount of NO2 needed to produce 25.0 kg of HNO3, we need to use the balanced chemical equation:
3 NO2(g) + H2O(l) ---> 2 HNO3(aq) + NO(g)
From the equation, we can see that one mole of HNO3 is produced for every 3 moles of NO2.
First, we need to calculate the molar mass of HNO3:
Molar mass of H = 1.0 g/mol
Molar mass of N = 14.0 g/mol
Molar mass of O = 16.0 g/mol
Total molar mass of HNO3 = (1.0 g/mol × 1) + (14.0 g/mol × 1) + (16.0 g/mol × 3) = 63.0 g/mol
Next, we need to calculate the number of moles of HNO3 needed:
Given mass of HNO3 = 25.0 kg = 25,000 g
Molar mass of HNO3 = 63.0 g/mol
Number of moles of HNO3 = given mass / molar mass = 25,000 g / 63.0 g/mol
Now, using the stoichiometric ratio from the balanced equation (3 mol NO2 : 2 mol HNO3), we can determine the number of moles of NO2 needed:
Number of moles of NO2 = (number of moles of HNO3 × 3 mol NO2) / 2 mol HNO3
Finally, we convert the number of moles of NO2 to mass:
Mass of NO2 = number of moles × molar mass of NO2
Please note: The molar mass of NO2 is 46.0 g/mol.
Now, you can calculate the amount of NO2 needed to produce 25.0 kg of HNO3 using the above steps.
To find out how much NO2 (nitrogen dioxide) someone should start with in order to end up with 25.0 kg of HNO3 (nitric acid), we need to use the balanced chemical equation and the stoichiometry of the reaction.
Let's start by examining the balanced chemical equation:
3 NO2(g) + H2O(l) ---> 2 HNO3(aq) + NO(g)
From the equation, we can see that 3 moles of NO2 react to produce 2 moles of HNO3 and 1 mole of NO. This means that the ratio of NO2 to HNO3 is 3:2.
To determine the amount of NO2 needed, we can use the following steps:
Step 1: Convert the mass of HNO3 required to moles.
Since the molar mass of HNO3 is approximately 63.01 g/mol, we can calculate the number of moles of HNO3 as follows:
Number of moles of HNO3 = Mass of HNO3 / Molar mass of HNO3
= 25.0 kg * 1000 g/kg / 63.01 g/mol
Step 2: Use the stoichiometry of the reaction to find the amount of NO2 needed.
Since the ratio of NO2 to HNO3 is 3:2, the number of moles of NO2 is related to the number of moles of HNO3 as follows:
Number of moles of NO2 = (3/2) * Number of moles of HNO3
Step 3: Convert the moles of NO2 to grams.
To determine the mass of NO2 required, we can use the formula:
Mass of NO2 = Number of moles of NO2 * Molar mass of NO2
Given that the molar mass of NO2 is approximately 46.01 g/mol, we can calculate the mass of NO2 needed using the values obtained in Step 1 and Step 2.
By following these steps, you can calculate the amount of NO2 required to obtain 25.0 kg of HNO3.