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NeVarCopy of 2024 Spring Final Exam P4-P6 (5/29/2024) (5/30/2024)

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

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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 calcium sulfate:  CaSO4

100.09 g/mol

88.14 g/mol

84.31 g/mol

136.14 g/mol

Calculate the molar mass for acetic acid: C2H4O2

92.08 g/mol

120.12 g/mol

112.24 g/mol

60.06 g/mol

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]

4.98 mol C2H6O

674.45 mol C2H6O

1.22 mol C2H6O

0.57 mol 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]

0.01 mol CO2

0.535 mol CO2

0.35 mol CO2

0.10 mol 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 ?

50.1 mol C3H8

75.0 mol C3H8

8.33 mol C3H8 

41.6 mol C3H8

Given the balanced equation:   2 SO2   +    O2  + 2 H2O   ------>      2 H2SO4
 How many moles of H2SO4 are produced from 16.3 moles of H2O ?

.125 mol H2SO4

32.6 mol H2SO4

16.3 mol H2SO4

12.5 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 13.5 g of H2 reacts, what mass of NH3 is formed?

342 g NH3

34.2 g NH3

152 g NH3

75.9 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?

0.00278 mol

0.10 mol

0.000556 mol

0.000278 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?

0.0278 L or 27.8 mL

0.0142 L or 14.2 mL

0.0139 L or 13.9 mL

0.000556 L or 0.556 mL

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?

0.2135 mol Asp

2.135 mol Asp

0.000854 mol Asp

0.00854 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.]

3009 mg aspirin in the tablet

150.2 mg aspirin in the tablet

1509 mg aspirin in the tablet

1539 mg aspirin in the tablet