Question

25 points , hi! please look at the attachment for the question, I'm having a hard time because all I have to do is solve through those 2 problems but I'm not sure if I solve the fractions first then multiply that result by 100 or what. I asked my teacher which she helped a little but I don't think she understood where I was lost. If you can help I would really appreciate it. Thank you.

This was the set up question:
4. If 100.0g of nitrogen gas (N2) is reacted with 100.0g of hydrogen gas (H2) to form NH3. What is the limiting and excess reactants?
Hint: Convert grams to moles for each reactant and then convert to moles of NH3. You need your balanced equation from answer 1 to determine the mole relationship between each reactant and the product NH3. Use the periodic table to determine the molar mass of all chemical formulas. Fill in the “?” blanks below to show your work.

and in the screenshot it has everything I'm working with and the conclusions I need to draw from it, I can draw the conclusions just fine on my own but I need help solving.

Answer 1

Step-by-step explanation:

Did u ever get answer

Answer 2

To answer the question, we correctly fill the attached screenshot as follows;

• 3H₂ + N₂ → 2NH₃
• The molar mass of H₂ = 2 g/mol

`100.0 g \ H_2 * (1 \ mol \ H_2)/(2 \ g \ H_2) * (2 \ mol \ NH_3)/(3 \ mol \ H_2) = 33.\bar 3 \ mol \ NH_3`

The molar mass of N₂ = 28 g/mol

`100.0 g \ N_2 * (1 \ mol \ N_2)/(28 \ g \ N_2) * (2 \ mol \ NH_3)/(1 \ mol \ N_2) \approx 7.143 \ mol \ NH_3`

A. Therefore, the excess reactant is hydrogen gas H₂ because it makes the most amount of ammonia, NH₃ (33.
`\bar 3` moles of NH₃)

B. The limiting reactant in nitrogen, N₂, because it is the reactant that makes the least amount of the ammonia, NH₃ (approximately 7.143 mol NH₃)

C. The theoretical yield of ammonia, is the maximum amount of ammonium that can be produced from the reaction between the 100 g of hydrogen gas, H₂, and 100 g of nitrogen gas, N₂ which is given by the amount of ammonia produced by the limiting reactant which is approximately 7.143 mole of NH₃

Step-by-step explanation: