Test 3 Quiz Questions Flashcards by Morgan Harrison

What is the mass % of H in C9H10N2?

Options:
1) 6.11%
2) 6.90%
3) 8.12%
4) 11.5%
5) 19.2%

2) 6.90%

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What is the mass % of carbon in ethanol: C2H5OH?

Options:
1) 26.06%
2) 53.29%
3) 26.65%
4) None of these
5) 52.13%

5) 52.13%

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What is the mass % of C in C9H10N2?

Options:
1) 49.5%
2) 69.4%
3) 91.1%
4) 19.2%
5) 73.9%

5) 73.9%

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What is the mass % of N in C9H10N2?

Options:
1) 23.4%
2) 28.2%
3) 19.2%
4) 15.7
5) 25.7%

3) 19.2%

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What is the empirical formula of a compound that contains 77.55% Xe and 22.45%F by mass?

XeF2

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What is the empirical formula of a compound that contains 63.25% Xe and 36.66%F by mass?

XeF4

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What is the empirical formula of a compound that contains 81.59% Cl and 18.41%O by mass?

Cl2O

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What is the empirical formula of a compound that contains 71.40% Br and 28.60%O by mass?

BrO2

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What is the empirical formula of a compound with the following mass percentages of carbon, hydrogen and nitrogen? C = 70.54% H = 13.02% and N = 16.45%

Options:
1) C6H7N
2) C5H11N
3) C3H4N
4) C5H13N
5) C5H12N2

2) C5H11N

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What is the empirical formula of a compound with the following mass percentages of carbon, hydrogen and nitrogen? C = 66.63% H = 7.46% and N = 25.91%

Options:
1) C6H7N
2) C5H11N
3) C5H12N2
4) C5H13N
5) C3H4N

5) C3H4N

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A substance is found to contain 73.14% C, 7.37% H and 19.49% O by mass. What is its empirical formula?

Options:
1) C4H8O
2) C5H6O
3) C3H8O
4) C6H12O

2) C5H6O

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Math question:

What mass of ammonium sulfate ((NH4)2SO4 132.15 g/mol) is required to produce 147 mL of a 2.50M solution of ammonium sulfate?

48.57

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Math question:

What is the concentration (in M) of a calcium nitrate (Ca(NO3)2 164.10 g/mol) solution prepared by dissolving 17.3 g of Ca(NO3)2 (164.10 g/mol) in enough water to produce 378 mL of solution? (Do not drop significant digits.)

0.279

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Math question:

What mass of copper (II) acetate (Cu(C2H3O2)2 141.64 g/mol) is required to produce 500.0 mL of a 1.18M solution of copper(II) acetate?

83.57

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Math question

What is the concentration (in M) of a sodium chloride(NaCl) solution prepared by dissolving 14.9 g of NaCl (58.44 g/mol) in enough water to produce 470 mL of solution? (Be careful not to drop significant digits.)

0.542

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Math question

Assuming volumes are additive, how much water (in mL) should be added to 12.4 mL of a 1.68 M solution of hydrochloric acid (HCl) to produce a 0.100 M solution?

195.92

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Math question:

What volume (in mL) of 7.38 M sodium chloride is required to produce 100.0 mL of a 0.496M solution?

6.72

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Math question:

Assuming volumes are additive, how much water (in mL) should be added to 18.9 mL of a 2.08 M solution of sodium hydroxide (NaOH) to produce a 0.250 M solution?

138.35

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Math question:

What is the concentration (in M) of a 2.36 M solution that is diluted from 28.9 mL to 500.0 mL?

0.136

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Math question:

What is the concentration of fluoride ions (in M) in a 8.83 M solution of cobalt(III) fluoride: CoF3

26.5

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Math question:

What is the molar concentration of Cr3+ ion in an aqueous solution of 0.443 M Cr2(SO4)3?

0.886

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Math question:

What is the concentration of iron ions (in M) in a 8.96 M solution of Fe3(PO4)2?

26.9

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Math question:

What is the molar concentration of SO42- ion in an aqueous solution of 0.223 M Cr2(SO4)3?

0.669

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What is/are the products of the combustion reaction of magnesium? Choose all correct answers.

Options:
1) CO2
2) MgO
3) O2
4) H2O

2) MgO

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What is/are the products of the combustion reaction of ethanol (C2H5OH)? Choose all correct answers. Options: 1) H2CO3 2) CO2 3) H2O 4) O2

2) CO2 3) H2O

What is/are the products of the combustion reaction of phosphorus? Choose all correct answers. Options: 1) H2O 2) CO2 3) P2O5 4) H3PO4

3) P2O5

What is/are the products of the decomposition of K2CO3? Choose all correct answers Options: 1) K2O 2) CO2 3) CO3 4) H2O

1) K2O 2) CO2

What is the formula of the precipitate formed from the precipitation reaction of Pb(NO3)2 and NaI?

PbI2

When aqueous solutions of NaI and AgNO3 are mixed, what precipitate(s) will form? Options: 1) no precipitate will form 2) AgI and NaNO3 3) NaNO3 4) AgI

4) AgI

What is the formula of the precipitate formed from the precipitation reaction of NaOH and AgNO3?

AgOH

When aqueous solutions of (NH4)3PO4 and KOH are mixed, what precipitate(s) will form? Options: 1) no precipitate will form 2) K3PO4 3) NH4OH 4) NH4OH and K3PO4

1) no precipitate will form

What is the formula of the precipitate formed from the precipitation reaction of Li2CO3 and ZnCl2?

ZnCO3

What are the spectator ions in the following reaction? (Choose all that apply) Cu(s) + 2AgNO3(aq) → 2Ag(s) + Cu(NO3)2(aq) Options: 1) no spectator ions present 2) Ag+ 3) Cu2+ 4) NO3-

4) NO3-

What are the spectator ions in the following reaction? (Choose all that apply) HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq) Options: 1) Cl- 2) OH- 3) H+ 4) Na+

1) Cl- 4) Na+

What are the spectator ions in the following reaction? (Choose all that apply) Ba(NO3)2(aq) + Na2CO3(aq) → BaCO3(s) + 2NaNO3(aq) Options: 1) Ba2+ 2) NO3- 3) Na+ 4) CO32-

2) NO3- 3) Na+

What is the oxidation number of Cr in CaCr2O7? Options: 1) +5 2) +4 3) +3 4) +6 5) +2 6) +1

4) +6

What is the oxidation number of H in BeH2? Options: 1) -2 2) +1 3) +2 4) -1

4) -1

True or False The following is an oxidation-reduction reaction: H2CO3(aq) → CO2(g) + H2O(l)

False

True or False The following is an oxidation-reduction reaction: CH4(g) + O2(g) → CO2(g) + H2O(g)

True

True or False The following is an oxidation-reduction reaction: Ba(NO3)2(aq) + Na2CO3(aq) → BaCO3(s) + 2NaNO3(aq)

False

True or False The following is an oxidation-reduction reaction: KClO4(s) → KCl(s) + 2O2(g)

True

What is the reducing agent in the following reaction? Cr(NO3)3(aq) + Al(s) → Al(NO3)3(aq) + Cr(s) Options: 1) Al(NO3)3 2) Cr(NO3)3 3) Al 4) Cr

3) Al

What species is undergoing reduction in the following reaction? NO3-(aq) + 4Zn(s) + 7OH-(aq) + 6H2O(l) → 4Zn(OH)42-(aq) + NH3(aq) Options: 1) NH3 2) NO3- 3) Zn 4) H2O 5) Zn(OH)42- 6) OH-

2) NO3-

What is the oxidizing agent in the following reaction? 5H2C2O4(aq) + 2KMnO4(aq) + 6HCl → 2MnCl2(aq) + 2KCl(aq) + 10CO2(g) + 8H2O(l) Options: 1) CO2 2) KCl 3) HCl 4) KMnO4 5) MnCl2 6) H2O 7) H2C2O4

4) KMnO4

Math Question: How many moles of oxygen will react with 14.6 moles of ethane according to the following reaction? 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

51.1

Math question: How many moles of carbon will react with 15.1mol of iron(III) oxide according to the following reaction? 2Fe2O3 + 3C → 4Fe + 3CO2

22.7

Math question: If 24.7mol of carbon dioxide is produced in the reaction below, how many moles of water is also produced? 2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

37.1

Math question: How many moles of carbon dioxide will be produced from the complete reaction of 16.1 mol of iron(III) oxide according to the following reaction? 2Fe2O3 + 3C → 4Fe + 3CO2

24.2

Math question: What mass of oxygen will react with 18.6 g of aluminum according to the following reaction? 4 Al + 3 O2 → 2 Al2O3

16.5

Math question: When 8.86 g of aluminum reacts with excess oxygen according to the following reaction, how many grams of aluminum oxide can be produced? 4 Al + 3 O2 → 2 Al2O3

16.7

Math question What mass of aluminum oxide can be recovered from the complete reaction of 32.1 g of Al with 32.1 g of oxygen gas? 4 Al (s) + 3 O2(g) → 2 Al2O3(s)

60.7

Math question What is the maximum number of grams of NO (30.01 g/mol) that can be formed from the reaciton of 16.8 g of NH3 (17.03 g/mol) with 24.4 g of O2 (32.00 g/mol)? 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l)

18.3

Math question If 44.6 g of iron(III) oxide and 19.3 g of carbon react, what is the theoretical yield in grams of iron metal? 2 Fe2O3(s) + 3 C(s) → 4 Fe (s) + 3 CO2(g)

31.2

What is the maximum theoretical number of moles of aluminum oxide that can be recovered from the reaction of 29.2 mol of aluminum and 27.2 moles of oxygen gas? 4 Al (s) + 3 O2(g) → 2 Al2O3(s)

14.6

If 14.4 moles of Cu and 16.2 moles of HNO3 are allowed to react, what is the maximum number of moles of NO that can be produced? 3 Cu + 8 HNO3 → 3Cu(NO3)2 + 2NO + 4H2O

4.05

If 3.3 moles of Al and 2.5 moles of Fe2O3 are allowed to react, what is the maximum number of moles of Al2O3 that can be produced? 2Al + Fe2O3 → Al2O3 + 2Fe

1.7

If 14.6 mol of iron(III) oxide and 17.5 mol of carbon react, what is the maximum number of moles of iron that can be recovered from the reaction? 2 Fe2O3(s) + 3 C(s) → 4 Fe (s) + 3 CO2(g)

23.3

If 11.4 mol of iron(III) oxide and 21.4 mol of carbon react, how many moles of the excess reactant will remain after the reaction? 2 Fe2O3(s) + 3 C(s) → 4 Fe (s) + 3 CO2(g)

4.3

What is the amount (in moles) of excess reactant remaining if all of the limiting reactant completely reacts when 25.9 mol of aluminum and 27.6 moles of oxygen gas react? 4 Al (s) + 3 O2(g) → 2 Al2O3(s)

8.2

If 12.1 moles of Cu and 44.8 moles of HNO3 are allowed to react, how many moles of excess reactant will remain if the reaction goes to completion? 3 Cu + 8 HNO3 → 3Cu(NO3)2 + 2NO + 4H2O

12.5

If 8.7 moles of Al and 2.7 moles of Fe2O3 are allowed to react completely, how many moles of the excess reactant will remain? 2Al + Fe2O3 → Al2O3 + 2Fe

3.3

Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3 (aq) + Na2SO4 (aq) --> Ag2SO4 (s) + 2 NaNO3 (aq) If 3.80 moles of AgNO3 and 3.05 moles of Na2SO4 are present initially, how many moles of excess reactant will remain after precipitation is complete? Write your answer to 2 decimal places.

1.15

Silver sulfate is precipitated from solution according to the following reaction 2 AgNO3 (aq) + Na2SO4 (aq) --> Ag2SO4 (s) + 2 NaNO3 (aq) If 8.07 moles of AgNO3 and 3.80 moles of Na2SO4 are present initially, how many moles of excess reactant will remain after precipitation is complete? Write your answer to 2 decimal places.

0.47

If ammonia can be produced from calcium oxide and ammonium chloride according to the following reaction. If 19.2 g of calcium oxide is used in the reaction and 6.28 g of ammonia is recovered, what is the % yield of the reaction? CaO(s) + 2 NH4Cl(s) → 2 NH3(g) + CaCl2(s) + H2O(g)

53.8

If 6.45 g of Mg undergoes the following reaction, what is the % yield if 6.76 g of magnesium nitride is produced? 3 Mg(s) + N2(g) → Mg3N2 (s)

75.7

If 5.57 g of sodium carbonate is recovered from the decomposition of 1.15 g of sodium bicarbonate, what is the percent yield of the reaction? (Note: I messed up on this problem and the percent yield will be unrealistically large. You can still solve it but will get a number much larger than I intended.) 2 NaHCO3(s) → Na2CO3(s) + CO2(g) + H2O(l)

767.8

Sulfur hexafluoride can be synthesized by burning sulfur with fluorine. What is the percent yield of the reaction if 60.3 g of sulfur hexafluoride is recovered from the combustion of 22.8 g of sulfur? S8(s) + 24 F2(g) → 8 SF6 (g)

58.1

What volume (in mL!!!) of 1.44 M NaOH is required to react with 20.5 mL of 1.13 M citric acid according to the following reaction? H3C6H5O7 (aq) + 3NaOH (aq) → 3H2O(l) + Na3C6H5O7 (aq)

48.3

What is the concentration of an HCl solution if 162.8 mL of it reacts completely with 22.6 g of Na2CO3 (105.99 g/mol)? Na2CO3 (s) + 2 HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g)

2.62

What volume (in mL!!!) of 2.28 M HCl is required to react with 4.05 g of zinc (65.41 g/mol) according to the following reaction? Zn(s) + 2 HCl (aq) → ZnCl2(aq) + H2(g)

54.3

41.5 mL of aqueous 0.255 M Pb(NO3)2 is mixed with 38.5 mL of 0.415 M NaCl. The equation for the precipitate reaction is: Pb(NO3)2 (aq) + 2 NaCl (aq) --> PbCl2 (s) + 2 NaNO3 (aq) The concentration of Pb2+ ion in the solution is _____ M after the reaction is complete.

0.0324

40.3 mL of aqueous 0.255 M Pb(NO3)2 is mixed with 21.5 mL of 0.415 M NaCl. The equation for the precipitate reaction is: Pb(NO3)2 (aq) + 2 NaCl (aq) --> PbCl2 (s) + 2 NaNO3 (aq) How many moles of PbCl2 are formed?

0.00446

35.8 mL of aqueous 0.255 M Pb(NO3)2 is mixed with 19.1 mL of 0.415 M NaCl. The equation for the precipitate reaction is: Pb(NO3)2 (aq) + 2 NaCl (aq) --> PbCl2 (s) + 2 NaNO3 (aq) The concentration of NO3- ion in the reaction solution is _____ M.

0.333