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2024 Spring Final Exam P1P3 (5/28/2024)

Last updated 11 months ago

12 questions

Calculating Molar Mass

Required

5

Required

5

Grams to Moles Conversions

Required

5

Required

5

Moles to Moles Stoichiometry

Required

5

Required

5

Required

5

Mass to Mass Stoichiometry

Required

5

Quality Control Titration Scenario

Required

5

Required

5

Required

5

Required

5

Question 1

1.

Question 2

2.

Question 3

3.

Question 4

4.

Question 5

5.

Question 6

6.

Question 7

7.

Question 8

8.

Question 9

9.

Question 10

10.

Question 11

11.

Question 12

12.

Calculate the molar mass for magnesium carbonate:  MgCO3

100.09 g/mol

84.31 g/mol

40.08 g/mol

88.08 g/mol

Calculate the molar mass for decanoic acid: C10H20O2

128.08 g/mol

172.30 g/mol

72.12 g/mol

112.24 g/mol

Calculate the number of moles of sodium hydroxide that is present in 14.65 g of NaOH [use 41.00 g/mol as the molar mass for NaOH]

674.45 mol NaOH

2.49 mol NaOH

0.36 mol NaOH

4.98 mol NaOH

Calculate the number of moles of carbon dioxide that is present in 15.42 g of CO2 [use 44.01 g/mol as the molar mass for CO2]

5.35 mol CO2

0.535 mol CO2

0.350 mol CO2

0.0350 mol CO2

Given the balanced equation:  C3H8    +    5 O2    ------>      3 CO2     +     4 H2O   
How many moles of C3H8 are needed to produce 25 moles CO2 ?

8.33 mol C3H8 

41.6 mol C3H8

75.0 mol C3H8

18.75 mol C3H8

Given the balanced equation:   2 SO2   +    O2  + 2 H2O   ------>      2 H2SO4
 How many moles of H2SO4 are produced from 12.5 moles of SO2 ?

12.5 mol H2SO4

Not enough information to calculate

6.25 mol H2SO4

.125 mol H2SO4

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 ?

Not enough information to calculate

Hydrogen reacts with excess nitrogen as follows:  N2 (g)   +   3H2 (g)   ----->   2 NH3 (g)
If 27.0 g of H2 reacts, what mass of NH3 is formed?

342 g NH3

34.2 g NH3

152 g NH3

15.2 g NH3

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?

0.000278 mol

0.00278 mol

0.10 mol

0.000556 mol

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?

0.0142 L or 14.2 mL

0.000556 L or 0.556 mL

0.0139 L or 13.9 mL

0.0278 L or 27.8 mL

The actual titration you performed used 0.0417 L of 0.2 M NaOH. How many moles of aspirin in your actual sample are present?

0.00167 mol Asp

0.00834 mol Asp

0.000834 mol Asp

0.0167 mol Asp

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.]

150.2 mg aspirin in the tablet

300.9 mg aspirin in the tablet

1503 mg aspirin in the tablet

3009 mg aspirin in the tablet