1.0 g of hydrogen reacts completely with 19.0 g of fluorine. What is the percent by mass of hydrogen in the compound that is formed?
My answer: 5.2631578947368
1.0 / (1.0 + 19.0) = ?
Well, well. Looks like we have a chemistry question here! Let's put on our lab coats and dive in, shall we?
To find the percent by mass of hydrogen, we need to first calculate the total mass of the compound formed. The molar mass of hydrogen is approximately 1 g/mol, and the molar mass of fluorine is about 19 g/mol.
So, for every 1 g of hydrogen reacted, we have 19 g of fluorine reacted as well. Adding these masses together gives us a total mass of 20 g for the compound formed.
Now, let's find the mass of hydrogen in the compound. Since we started with 1 g of hydrogen, and the total mass is 20 g, we can conclude that the mass of hydrogen in the compound is still 1 g.
To find the percent by mass of hydrogen, we divide the mass of hydrogen in the compound (1 g) by the total mass of the compound (20 g) and then multiply by 100. Doing the math, we find:
(1 g / 20 g) * 100 = 5%
So, my friend, the percent by mass of hydrogen in the compound is approximately 5%. It seems like hydrogen is going incognito in this compound!
Keep those chemistry questions coming. I'll be here with my Bunsen burner and clown nose, ready to clown around!
To find the percent by mass of hydrogen in the compound formed, we first need to determine the molar masses of hydrogen and fluorine.
The molar mass of hydrogen (H) is approximately 1.01 g/mol.
The molar mass of fluorine (F) is approximately 19.0 g/mol.
Next, we need to determine the moles of hydrogen and fluorine involved in the reaction.
1.0 g of hydrogen divided by the molar mass of hydrogen (1.01 g/mol) gives us:
1.0 g / 1.01 g/mol = 0.9901 mol
19.0 g of fluorine divided by the molar mass of fluorine (19.0 g/mol) gives us:
19.0 g / 19.0 g/mol = 1.0 mol
Since the reaction between hydrogen and fluorine is in a 1:1 ratio, they completely react with each other. Therefore, the moles of hydrogen in the compound formed is the same as the moles of fluorine, which is 1.0 mol.
The total mass of the compound formed is the sum of the masses of hydrogen and fluorine:
Mass of compound = mass of hydrogen (1.0 g) + mass of fluorine (19.0 g) = 20.0 g
Now, we can calculate the percent by mass of hydrogen in the compound:
Percent by mass of hydrogen = (mass of hydrogen / mass of compound) x 100
= (1.0 g / 20.0 g) x 100
= 5.0%
Therefore, the percent by mass of hydrogen in the compound that is formed is 5.0%.
To calculate the percent by mass of hydrogen in the compound, you need to determine the total mass of the compound and the mass of hydrogen in the compound.
1. First, let's calculate the molar masses of hydrogen (H) and fluorine (F). The molar mass of hydrogen is approximately 1.01 g/mol, and the molar mass of fluorine is approximately 19.0 g/mol.
2. Determine the number of moles of hydrogen and fluorine in the given masses. To do this, divide the given masses by their respective molar masses:
Moles of hydrogen = 1.0 g / 1.01 g/mol ≈ 0.99 mol
Moles of fluorine = 19.0 g / 19.0 g/mol = 1.0 mol
3. Next, we need to determine the limiting reactant, which is the reactant that is entirely consumed in the reaction. In this case, hydrogen is the limiting reactant because it is present in a smaller amount compared to fluorine.
4. The balanced chemical equation for the reaction between hydrogen (H₂) and fluorine (F₂) is:
H₂ + F₂ → 2HF
According to the balanced equation, 1 mole of hydrogen reacts with 1 mole of fluorine to form 2 moles of hydrogen fluoride (HF). Since hydrogen is the limiting reactant, all of it will be consumed, and no excess hydrogen will be left.
5. Determine the mass of hydrogen in the compound formed. As we just determined, 0.99 moles of hydrogen react, so the mass of hydrogen in the compound is:
Mass of hydrogen = 0.99 mol * 1.01 g/mol ≈ 1.0 g
6. Finally, calculate the percent by mass of hydrogen in the compound using the following formula:
Percent by mass of hydrogen = (Mass of hydrogen / Total mass of the compound) * 100
Total mass of the compound = mass of hydrogen + mass of fluorine = 1.0 g + 19.0 g = 20.0 g
Plugging in these values:
Percent by mass of hydrogen = (1.0 g / 20.0 g) * 100 ≈ 5.0%
Therefore, the percent by mass of hydrogen in the compound formed is approximately 5.0%.