Calculate the molar mass for calcium sulfate: CaSO4
Calculate the molar mass for acetic acid: C2H4O2
Calculate the number of moles of ethanol (C2H6O) that is present in 26.45 g of [use 46.08 g/mol as the molar mass for C2H6O]
Calculate the number of moles of carbon dioxide that is present in 0.46 g of CO2 [use 44.01 g/mol as the molar mass for CO2]
Given the balanced equation: C3H8 + 5 O2 ------> 3 CO2 + 4 H2O
How many moles of C3H8 are needed to produce 16.7 moles CO2 ?
Given the balanced equation: 2 SO2 + O2 + 2 H2O ------> 2 H2SO4
How many moles of H2SO4 are produced from 16.3 moles of H2O ?
Given the balanced equation: 2 SO2 + O2 + 2 H2O ------> 2 H2SO4
Which is the correct mole ratio to calculate how many moles of O2 are needed to produce 12.5 moles H2SO4 ?
Hydrogen reacts with excess nitrogen as follows: N2 (g) + 3H2 (g) -----> 2 NH3 (g)
If 13.5 g of H2 reacts, what mass of NH3 is formed?
You will be using 0.2 M NaOH as your titrant solution. Your first job is to predict how many milliliters (mL) you are EXPECTING to use for the 500mg tablet. Use the molar mass of aspirin as 180.17 g/mol for ALL future calculations where molar mass is needed.
How many moles would be present in a 500 mg tablet?
Knowing that the mole ratio for the titration is 1 mol NaOH: 1 mol Asp, what volume of 0.2 M NaOH would be needed if the expected tablet is 500 mg?
The actual titration you performed used 0.0427 L of 0.2 M NaOH. How many moles of aspirin in your actual sample are present?
And finally, using your answer choice from #3, how many milligrams of aspirin was in the sample tablet from the same batch that made the person ill? [Note: If your answer from #3 is incorrect, but you do the calculation for this question correctly, I will count it as correct.]