I missed a few days of school due to a sick child. I'm reviewing for an exam and the following questions are giving me trouble as I wasn't there when they were reviewed in class. If possible, I need the step-by-step process. Thanks.
1.) If you put hydrogen peroxide on a cut, you’ll notice that it bubbles. The bubbles are diatomic oxygen which is effectively “sterilizing” the wound. If you had 10 g of H2O2, how many grams of oxygen would you form on the cut.
2.) Alka Seltzer is a solid mixture of sodium bicarbonate and citric acid that when placed in water undergoes this reaction…..fizzing.
3NaHCO3(s) + C6H8O7(s) = 3CO2(g) + 3H2O(l) + Na3C6H5O7(aq)
Who is the limiting reactant if you had 100g each of sodium bicarbonate and citric acid?
a. Pure H2O2?
mass O2=10 (2*16/(2(16+1))=10 (32/34)
b. figure moles of each
moles NaHCO3=100/molmass
moles acid=100/molmass
now, do you have three times the moles of bicarb as do you have of acid? (look at the equation coefficents).
If you have more than three times as much bicarb, then the limiting reactant is the acid.
Ah, this is what it means "below". In the second question I posted (above I guess) I rephrased my question for answer and all work. I'm really confused as to what your provided answer means as I missed these classes. I honestly have no idea what to make of the information you provided me, Sir.
I've tried to help at your other post.
Thank you so much. This is sure to be very helpful!
1.) To determine the number of grams of oxygen formed when 10 g of H2O2 is applied to a cut, you need to calculate the molar mass of H2O2 and then use stoichiometry.
Step-by-step process:
1. Calculate the molar mass of H2O2:
- Hydrogen (H) has a molar mass of 1 g/mol.
- Oxygen (O) has a molar mass of 16 g/mol.
- H2O2 consists of 2 hydrogen atoms and 2 oxygen atoms.
- Molar mass of H2O2 = (2 * molar mass of H) + (2 * molar mass of O)
2. Calculate the number of moles of H2O2:
- Given mass of H2O2 = 10 g
- Moles of H2O2 = mass of H2O2 / molar mass of H2O2
3. Use the stoichiometry of the reaction:
- According to the balanced chemical equation, 1 mol of H2O2 produces 1 mol of O2.
- Therefore, moles of O2 = moles of H2O2
4. Calculate the mass of oxygen:
- Mass of O2 = moles of O2 * molar mass of O
This step-by-step process will allow you to determine the number of grams of oxygen formed when 10 g of H2O2 is applied to a cut.
2.) To identify the limiting reactant when you have 100 g each of sodium bicarbonate (NaHCO3) and citric acid (C6H8O7), you need to compare the moles of each reactant and calculate the stoichiometry of the reaction.
Step-by-step process:
1. Calculate the molar mass of NaHCO3 and C6H8O7.
2. Calculate the number of moles of NaHCO3 and C6H8O7:
- Moles of NaHCO3 = mass of NaHCO3 / molar mass of NaHCO3
- Moles of C6H8O7 = mass of C6H8O7 / molar mass of C6H8O7
3. Use the stoichiometry of the reaction:
- According to the balanced chemical equation, 1 mol of NaHCO3 reacts with 1 mol of C6H8O7 to produce 3 mol of CO2, 3 mol of H2O, and 1 mol of Na3C6H5O7.
- Determine the ratio of moles of NaHCO3 to C6H8O7 in the reaction.
- Compare the actual moles of each reactant with the stoichiometric ratio.
4. Identify the limiting reactant:
- The reactant that has fewer moles compared to the stoichiometric ratio is the limiting reactant.
- The limiting reactant is the one that will be completely consumed in the reaction, limiting the amount of product formed.
By following this step-by-step process, you can determine which reactant is the limiting reactant when you have 100 g each of sodium bicarbonate and citric acid.