CHEM 1021 Lecture Notes - Lecture 25: Spectator Ion, Chemical Equation, Sodium Nitrate

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23 Oct 2016

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Clicker question 1: which of the following solutions when mixed with a solution of calcium chloride will produce a precipitate: aqueous sodium carbonate, cacl2 (aq) + na2co3 (aq) , aqueous sodium nitrate, cacl2 (aq) + nano3 (aq) . 2na^+ (aq) +2cl^- (aq: all the ions are spectators, no net ionic equations, cacl2(aq) + nano3(aq) ca(no3)2(aq) + nacl(aq, no reaction because there was no formation of a solid. Must include charges and state/phase on all reactants and products: ca^2+ (aq) + 2cl^- (aq) + 2na^+ (aq) + co3^2- (aq) 2na^+(aq) + 2cl^- (aq) , the net ionic equation. Caco3(s: eliminates the spectator ions and shows the actual chemical change taking place, must include charge and state/phase on all reactants and products, spectator ions: na^+, cl^, ca^2+ (aq) + co3^2- (aq) caco3 (s) Bacl2(aq) + na2so4(aq) baso4 (s) + 2nacl(aq: barium ion, chloride ion, sulfate ion, water. What is the other spectator ion: sodium ion.

Related Questions

Write (1) a balanced molecular equation, (2) a total ionic equation, and (3) a net ionic equation that would describe a predicted reaction. Please pay attention to details such as charges (e.g. Ba2+ vs. Ba) and states (i.e. (aq), (s), (l), or (g) as appropriate). If a reaction is not predicted to occur (soluble salts on both sides of the equation), only the balanced molecular equation is needed.

sodium carbonate + sulfuric acid

Na2CO3 (aq)+ H2SO4(aq) -> Na2SO4(aq) + CO2 (g)+ H2O(l)

Na+(aq)+CO3^2−(aq)+2H+(aq)+SO4^2−(aq) ->H2O(l)+CO2(g)+2Na+(aq)+SO4^2−(aq)

CO3^2−(aq)+2H+(aq) -> H2O(l)+CO2(g)

sodiumcarbonate + hydrochloric acid

Na2CO3(aq) + HCl (aq)-> NaCl (aq)+ H2O (l)+ CO2(g)

Na+(aq) + CO3^-2 (aq)

potassium chloride + sodium carbonate

KCl (aq)+ Na2CO3 (aq)-> K2CO3 (aq)+ 2NaCl(aq)

potassium chloride + silver nitrate

KCl (aq)+ AgNO3 (aq) -> KNO3 (aq)+ AgCl (s)

potassium chloride + sodium nitrate

KCl (aq)+ NaNO3 (aq) -> KNO3 (aq)+ NaCl(aq)

nickel chloride + silver nitrate

NiCl2 (aq)+ 2AgNO3(aq) -> Ni (NO3)2(aq) + 2AgCl (s)

nickel chloride + sodium carbonate

KCl (aq)+ Na2CO3(aq) -> K2CO3 (aq)+ 2NaCl(aq)

hydrochloric acid + sodium hydroxide

HCl (aq)+ NaOH(aq) -> NaCl(aq) + H2O(l)

Ammonium chloride + sodium hydroxide

NH4Cl(aq) + NaOH(aq) -> NaCl(aq) + H2O (l)+ NH3(g)

sodium acetate + hydrochloric acid

CH3COONa (aq)+HCl (aq) -> CH3COOH(aq) +NaCl(aq)

lead nitrate + sulfuric acid

Pb(NO3)2 (aq)+ H2SO4(aq) -> PbSO4 (aq)+ HNO3(aq)

oliveserval487

Balance the following Chemical Equations:

____Fe(s) + ____H₂O(g) Â® ____Fe₃O₄(s) + ____H₂(g)

____C₂H₆(g) + ____O₂(g) Â® ____CO₂(g) + ____H₂O(g)

___ C₆H₁₄ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (g)

___ C₃H₈O₃ (l) + ___ O₂ (g) Â® ___ CO₂ (g) + ___ H₂O (l)

___ NaN₃ (s) Â® ___ Na (s) + ___ N₂ (g)

__ C₃H₅N₃O₉ Â® __ CO₂ + ___ N₂ + ___ H₂O + ___ O₂

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H₂O(g) + C(s) â¶ CO(g) +H₂(g)

(B) 2KClO₃(s) â¶ 2KCl(s) +3O₂(g)

(D) Pb(NO₃)₂(aq) + H₂SO₄(aq) â¶ PbSO₄(s) + 2HNO₃(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H₃PO₄

(B) Al(OH)₃

6. Complete and balance the following acid-base equations:

(A) A solution of HClO₄ is added to a solution of LiOH.

(B) Aqueous H₂SO₄ reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)₂(aq) + HC₂H₃O₂(aq) â¶

(B) H₃PO₄(aq) + CaCl₂(aq) â¶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl₂ and H₂. Ans: 1.67 g Mg

9. H₂ is produced by the reaction of 118.5 mL of a 0.8775-M solution of H₃PO₄ according to the following equation: 2Cr + 2H₃PO₄ â¶ 3H₂ + 2CrPO₄. How many grams of H₂ are produced? Ans: .315 g H₂

10. Automotive air bags inflate when a sample of sodium azide, NaN₃, is very rapidly decomposed.

2NaN₃(s) â¶ 2Na(s) + 3N₂(g)

What mass of sodium azide is required to produce 2.6 ft³ (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN₃

11. Urea, CO(NH₂)₂, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO₂ produced by combustion of 1.00 x 10⁴ grams of CO₂?

CO₂(g) + 2NH₃(g) â¶ CO(NH₂)₂(s) + H₂O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H₂SO₄(l) â¶ HCl(g) + NaHSO₄(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO₃(s)â¶CaO(s) + CO₂(s)

Ans: 92.0 %

14. Citric acid, C₆H₈O₇, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C₁₂H₂₂O₁₁ + H₂O +3O₂ â¶2C₆H₈O ₇+ 4H₂O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P₄ and 0.200 mol of O₂ react according to P₄+5O₂ â¶ P₄O₁₀?

(B) Calculate the percent yield if 10.0 g of P₄O₁₀ is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N₂ â¶ Li₃N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO₃ requires 20.22 mL of the AgNO₃ solution to reach the end point?

AgNO₃(aq) + NaCl(aq) â¶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO₃)₂ solution.

2Cl^â(aq) + Hg(NO₃)₂(aq) â¶ 2NO₃^â(aq) + HgCl₂(s)

What is the Cl^â concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO₃)₂(aq) to reach the end point?

Ans: 0.009636 M

Having trouble with thse questions. Please answer all questions correctly. Will provide a thumbs up.

1.Which of these equations is the balanced reaction between nitrous acid solution and solidmagnesium hydroxide ?

A.2NH₃(aq) + MgOH (s) Mg(NH₄)₂(aq) + 2 H₂O(l)

B.2HNO₂(aq) + Mg(OH)₂(s) Mg(NO₂)₂(aq) + 2 H₂O(l)

C.2HNO₃(aq) + Mg(OH)₂(s) Mg(NO₃)₂(aq) + 2 H₂O(l)

D.2HNO₂(aq) + MgOH (s) Mg(NO₃)₂(s) + 2H₂O(l)

2.Balance the following chemical equation:

C₃H₇OH(l) + O₂(g)CO₂(g) + H₂O(g)

a. C₃H₇OH(l) + 4 O₂(g)3 CO₂(g) + 4 H₂O(g)

b.2 C₃H₇OH(l) + 9 O₂(g)6 CO₂(g) + 8 H₂O(g)

c.C₃H₇OH(l) + 5 O₂(g)3 CO₂(g) + 4 H₂O(g)

d.C₃H₇OH(l) + O₂(g)CO₂(g) + H₂O(g)

3.Which species would be considered a spectator ion based on the following equation?

Ba²⁺ + 2NO₃^â + 2Na⁺ + SO₄^2- â BaSO₄(s) + 2NO₃^â + 2Na⁺

SO₄^2-

2NO₃^â

Ba²⁺

BaSO₄

4.Barium sulfate is often ingested to aid in the diagnosis of GI tract disorders. The equation for its production is Ba²⁺ + SO₄^2- â BaSO₄(s). What type of equation is this?

A full equation

A net ionic equation

A total ionic equation

An oxidation-reduction equation

5.Which species is being reduced in this reaction?

CuO(s) + H₂(g) Cu(s) + H₂O(g)

H₂O

CuO

H₂

6.Which of the following is an oxidizing agent?

H₂

NH₃

O₂

H₂O

7.The following chemical equation,

HC₂H₃O₂(aq) + KOH(aq) KC₂H₃O₂(aq) + H₂O(l),

is an example of a(n) _______ reaction.

a.oxidation-reduction and acid-base

b.acid-base

c.precipitation

d.oxidation-reduction and precipitation

e.oxidation-reduction

8.What substance is oxidized in the following reaction?

4HCl + MnO₂ â Cl₂ + 2H₂O + MnCl₂

a.Mn in MnO₂

b.O in MnO₂

c.Cl in HCl

d.H in HCl

9.What is the reducing agent in the following reaction?

4HCl + MnO₂ â Cl₂ + 2H₂O + MnCl₂

Cl₂

MnCl₂

HCl

MnO₂

10.All redox reactions involve oxygen.

True

False

11.The term formula weight can be used with respect to which of the following?

A.ionic compounds

B.covalent compounds

C.both a and b

D.neither a nor b

12.What is the molecular weight of ibuprofen, C₁₃H₁₈O₂?

A.206.3 amu

B.377.7 amu

C.29.0 amu

D.289.4 amu

13.The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A.a sample which weighs exactly 12 atomic mass units

B.a sample which contains 6.02 Ã 10²³ atoms of ¹²C

C.both a and b

D.neither a nor b

14.The mass of an atom of ¹²C is exactly 12 atomic mass units. Which of the following describes a mole of ¹²C atoms?

A.a sample which contains 6.02 Ã 10²³ atoms of ¹²C

B.a sample which weighs exactly 12.011 grams

C.both a and b

D.neither a nor b

15.What is the molar mass of water, H₂O?

A.18.02 g

B.18.02 amu

C.17.01 g

D.17.01 amu

16.What is the molar mass of glucose, C₆H₁₂O₆?

A.180.2 amu

B.180.2 g

C.60.05 amu

D.60.05 g

17.In the reaction 2H₂O â 2H₂ + O₂, 2.0 mol water will produce how many grams of O₂?

18.In the reaction 2CH₄ + O₂ â 2CO + 4H₂, how many molecules of CO will be produced by the complete reaction of 1.60 grams of CH₄?

3.01 Ã 10²²

2.00

12.0 Ã 10²³

6.02 Ã 10²²

19.Suppose 2.43 g of magnesium is reacted with 3.20 g of oxygen: 2Mg + O₂ â 2MgO. How many grams of MgO will be produced?

1.27

4.03

5.63

8.06

20.Which of the following conversion factors would allow one to calculate the amount of PbI₂produced from a given amount of NaI in the following unbalanced reaction?

Pb(NO₃)₂ + Nal â Pbl₂ + NaNO₃

21.The unbalanced equation for the reduction of copper(I) sulfide with oxygen is given below. What mass of copper is produced from the reduction of 7.50 g Cu₂S?

Cu₂S(s) + O₂(g) Cu(s) + SO₂(g)

18.8 g

5.99 g

1.50 g

9.39 g

2.99 g

22.How many grams of aluminum oxide are produced by the complete reaction of 19.8 g aluminum with excess oxygen?

10.5 g aluminum oxide

37.4 g aluminum oxide

49.9 g aluminum oxide

74.8 g aluminum oxide

23.If 5 grams of CO and 5 grams of O₂ are combined according to the reaction, which is the limiting reagent?

2CO + O₂ â 2CO₂

O₂

CO and O₂

CO₂

24.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 26%. How much hydrogen is needed to produce 4.8 kg ammonia?

1.5 kg

7.0 kg

0.85 kg

3.3 kg

25.A percentage yield greater than 100% has been reported in a scientific paper you are assigned to read. What would be a reasonable explanation for this?

a. The product was measured more than once.

b. It must be a typographical error since yields can't exceed 100%.

c. A lack of training of the professor who published the study.

d. Small measurement errors could have caused this to occur.

26.In an industrial process, nitrogen is reacted with hydrogen to produce ammonia. The percent yield of this particular process is 24.8%. How much hydrogen is needed to produce 3.7 kg ammonia?

1.8 kg

1.2 kg

4.4 kg

12 kg

2.7 kg

27.The following reaction has a percent yield of 90.5%. How many grams of carbon dioxide are produced from 78.5 g calcium carbonate via this reaction?

2 HNO₃(aq) + CaCO₃(aq) Ca(NO₃)₂(aq) + H₂O(l) + CO₂(g)

34.5 g

21.6 g

38.1 g

31.2 g

28.When gas molecules dissolve in liquids to form a saturated system, the process is usually

exothermic.

endothermic.

independent of the nature of the liquid.

temperature independent.

29.The reaction below would be considered.

CaCO₃ + heat â CaO + CO₂

an exothermic combination.

an exothermic decomposition.

an endothermic combination.

an endothermic decomposition.

30.The combustion of one mole of propane, C₃H₈, releases 531 kcal. How much heat is released by the combustion of 1.20 moles of propane?

A.584 kcal

B.690 kcal

C.443 kcal

D.637 kcal

31.The combustion of one mole of propane, C₃H₈, releases 531 kcal. How much heat is released by the combustion of 4.40 g of propane?

A.531 kcal

B.5.31 Ã 10⁴ kcal

C.53.1 kcal

D.5.31 Ã 10³ kcal

32.Metabolism of one mole of glucose, C₆H₁₂O₆, releases 670 kcal. How much heat is released by the combustion of 0.300 moles of glucose?

A.201 kcal

B.2.41 Ã 10³ kcal

C.186 kcal

D.2.23 Ã 10³ kcal

33.Metabolism of one mole of glucose, C₆H₁₂O₆, releases 6.70 Ã 10² kcal. How much heat is released by the combustion of 50.0 g of glucose?

A.201 kcal

B.2.41 Ã 10³ kcal

C.186 kcal

D.2.23 Ã 10³ kcal

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CHEM 1021 Lecture Notes - Lecture 25: Spectator Ion, Chemical Equation, Sodium Nitrate

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