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13 Dec 2019

Ammonia gas combines with oxygen gas to produce liquid water and nitrogen gas. a) Write a balanced equation for the equilibrium reaction b) Write the expression for the equilibrium constant c)Calculate Keq if the equilibrium concentrations of the following components are: [NH3]=0.3M; [O2]=0.5M; [H2O]=55.6M; [N2]=2.0M d) Experiments show that this reaction is endothermic, what effect will raising the temperature have on the position of equilibrium? Explain. Explain why a reaction reaches equilibrium and why we refer to it as a dynamic equilibrium.

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Nestor RutherfordLv2

16 Dec 2019

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Pre-Laboratory Question: Investigating Chemical Reactions

Balance each of the following equations, and classify each of the reactions by type.

Reaction Equation

Type of Reaction

KClO₃

KCl

O₂

Na₂O₂

Pb(NO₃)₂

KNO₃

PbI₂

AgNO₃

Cu(NO₃)₂

C₃H₈

O₂

CO₂

H₂O

Heat

HCl

ZnCl₂

H₂

Laboratory Questions

Activity 1: Synthesis Reaction

Describe all of the signs that indicated a chemical reaction occurred.

Describe the temperature change that occurred during this reaction. Is heat required or produced during the reaction?

Describe any other changes that were observed in the steel wool. What reaction might create such a change?

Write a balanced equation for the reaction of the steel wool with oxygen. Be sure to include heat energy in the reaction.

Activity 2: Decomposition Reaction

What gases could be produced from decomposing hydrogen peroxide?

Which gas was produced?

Write a balanced equation for the decomposition of hydrogen peroxide.

Activity 3: Single-Replacement Reaction

What gases could be produced from hydrochloric acid (HCl)?

Which gas was produced?

Write a balanced equation for the reaction of magnesium with hydrochloric acid.

Why did you need to tilt the splint at a 45-degree angle?

a. Write a balanced equation for the reaction initiated by the burning splint.

b. Classify the reaction initiated by the burning splint.

Activity 4: Double-Replacement Reaction

Describe the reaction of sodium bicarbonate and vinegar.

Refer to the section in the Background titled, âStandard Tests Gaseous Products.â Use a flaming splint and a glowing splint to identify the gas above the liquid in the cup. Write the name and formula of the gas in the space provided.

Write a balanced chemical equation for this double-replacement reaction.

One of the two products of this reaction is carbonic acid (H₂CO₃), which immediately forms water and the gas you identified after exposure to the flaming and glowing splints. Write a balanced equation showing the decomposition of carbonic acid.

Activity 5: Combustion Reaction

Explain why water appears on the inside of the glass test tube.

Write a balanced equation for the combustion reaction.

Activity 6: Precipitation Reaction

Write a balanced equation for the precipitation reaction.

Which product in the above reaction is the precipitate?

Discussion Questions

Predict the product(s) of the following equations. Balance the equations, and classify each of the reactions by type.

Equation

Type of Reaction

Pb(NO₃)₂ + Na₂CO₃ â

C₄H₁₀

O₂

Zn + CuSO₄

CaCO₃

Heat

H₂O

O₂

MgSO₄

LiOH

NiSO₄

SO₂ + H₂O â

10.

HgO

Heat

Nitric acid may be produced by oxidizing ammonia to nitric oxide over a platinum-rhodium catalyst, then oxidizing the nitric oxide to nitrogen dioxide in a separate unit where it is absorbed in water to form an aqueous solution of nitric acid. The three key reactions in the synthesis are the oxidation of the ammonia to nitric oxide and of nitric oxide to nitrogen dioxide, followed by dissolution of the NO₂ in water:

4NH₃(g)+ 5O₂(g)â 4NO(g)+ 6H₂O(g)

2NO(g) + O₂(g) â 2NO₂(g)

4NO₂ (g)+ 2H₂O(l) + O₂(g) â 4HNO₃(aq)

In this problem, you may neglect side reactions that would lower the product yield. This would include the side reaction in which ammonia is oxidized to form nitrogen and water which can lower product yield.

4NH₃ + 3O₂ â 2N₂ + 6H₂O

Thus, for this project the overall reaction may be represented from the three key reactions above as:

NH₃ + 2O₂ â H₂O + HNO₃

Ammonia vapor at 275^oC and 8 atm is mixed with air, also at 275^oC and 8 atm, and the combined stream is fed to a converter. Fresh air entering the system at 30^oC and 1 atm with a relative humidity of 50% is compressed to 100^oC and 8 atm, and the compressed air then exchanges heat with the product gas leaving the converter. The quantity of oxygen in the feed to the converter is 20% in excess of the amount theoretically required to convert all the ammonia to HNO₃. The entire process after the compressor may be taken to operate at a constant pressure of 8 atm.

In the converter, the ammonia is completely oxidized, with a negligible amount of NO₂ formed. The product gas leaves the converter at 850^oC and exchanges heat with the air leaving the system as described earlier. The product gas is then fed to a waste-heat boiler that produces superheated steam at 200^oC and 10 bar from liquid water at 35^oC. The product gas leaving the waste-heat boiler is cooled further to 35^oC and fed to an absorption column in which the NO is completely oxidized to NO₂ which in turn combines with water (some of which is present in the product gas). Water is fed to the absorber at 25^oC, at a rate sufficient to form a 55 wt% aqueous nitric acid solution. Any NO formed in the reaction of NO₂ to produce HNO₃ is oxidized and the NO₂ produced is hydrated to form still more HNO₃. The off-gas from the process may be taken to contain only N₂ and O₂ and at 25^oC and 1 atm.

b). Taking a basis of 100 kmol of ammonia fed to the process

(i) kmol of water fed to the absorber

(ii). Temperature of the product gas after it has exchanged heat with the air, assuming no heat is transferred between the heat exchanger and the surroundings

SCH3U U1 Experiment #10 DecompositionReactions

Purpose:

To observe four decompositionreactions.

Hypothesis:

Part A:

Lead (II) Nitrate > Lead +Nitrogen Gas + Oxygen Gas

Part B:

Hydrogen Peroxide > Water + OxygenGas

Part C:

Ammonium Carbonate > Ammonia +Carbon Dioxide

Part D:

Copper (II) Carbonate > CopperOxide + Carbon Dioxide

Materials:

See experiment handout. U1 Experiment#10 Decomposition Reactions

Procedure:

See experiment handout. U1 Experiment#10 Decomposition Reactions

Part D: (teacherdemonstration)

1)Heat a small amount of CopperCarbonate in a test tube over a Bunsen burner.

2)Collect the gas produced and bubblethrough lime water.

Observations:

PartA:

Lead (II) Nitrate --pale yellow finedull powder

Glowing splint test-- reignited

Burning splint test-- brightened

--brown gas was produced (NitrogenDioxide)

Part B:

Hydrogen Peroxide-- clear, colorlessliquid

Magnesium (IV) Oxide-- fine blackpowder

Flaming splint test-- wasextinguished

Glowing splint test-- reignitessplint

Reaction: reacts vigorouslyproducing a gas, dark powder mixed throughout. Reaction continuedfor several minutes.

Part C:

Ammonium Carbonate-- fine dull whitepowder

Red litmus-- turned blue

Blue litmus-- stayed blue

Dried cobalt paper-- turned pink

Glowing splint test--extinguished

Burning splint test--extinguished

Part D:

Copper Carbonate-- dull green-bluefine powder

Lime water-- clear liquid

Results of lime water test: Limewater turned cloudy and milky, and a precipitate formed in limewater.

CuCO₃ turns black as thereaction occurs.

Conclusion:

Four decompositions reactions wereobserved. In all of the experiments gases were produced.

Discussion:

1)The balanced equations are:

Part A:

2Pb(NO₃)₂ >4NO₂ + 2PbO + O₂

Part B:

H₂O₂ >H₂ + O₂

Part C:

(NH₄)₂CO₃ > 2NH₃ +CO₂ + H₂O

Part D:

CuCO₃ > CO₂+ CuO

2) The gas produced though thedecomposition of compounds containing the carbonate ion is carbondioxide (CO₂).

3) There are many tests to confirmthe presence of different gases. To test for CO₂ you canbubble the gas through lime water and it should turn cloudy ormilky. To test for O₂ you can place a glowing splint inthe gas and it should ignite. The presence of NH₃ can beconfirmed by it's ability to extinguish a glowing or flamingsplint, also it turns red litmus paper blue, and has a distinctivepungent odor. The presence of water vapor can be confirmed withcobalt paper, which turns pink when contacted by water vapor.Hydrogen gas (H₂) is tested for by placing a flamingsplint in the unknown gas, and a popping sound will be heard, thesplint will also be extinguished.

4) A balanced chemical equation forammonium gas and water is:

NH₃ + H₂O >NH₄⁺_(aq) +OH^-_(aq)

This explains why NH₃causes red litmus paper to turn blue, as the products areNH₄⁺ + OH^- , and OH^- isan indicator of a base, and bases turn red litmus paper blue. Thishappens because as the ammonium gas contacts the moist litmus paperit reacts with the water that has moistened the paper beforeeffecting the litmus paper.

5) A balanced chemical equation forcarbon dioxide and water is:

CO₂ + H₂O >H₂CO_3(aq)

The product is carbonic acid, andacids turn moist litmus paper red. The carbon dioxide reacts withthe water held by the litmus paper before reacting with the litmuspaper so is acidic when affecting the paper.

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