1. Consider this reaction:

H₂(g) +    O₂ (g)     à       H₂O (g)                                          dHo = __________

1. Balance the equation and put the correct number of moles in the equation above. (1 point)

2. Classify the forward reaction as (1) Combustion, (2) Decomposition, (3) Single replacement, (4) Double replacement, (5) Neutralization, (6) Synthesis. Circle the correct answer. (1 point)

3. In this reaction did Hydrogen get oxidized or reduced? Circle the correct answer. (1 point)

4. Based on your answer above is Hydrogen an oxidizing or reducing reactant? Circle the correct answer. (1 point)

5. In this reaction did Oxygen get oxidized or reduced? Circle the correct answer. (1 point)

6. Based on the answer above, is Oxygen an oxidizing or reducing agent? Circle the correct (1 point)
   
7. Calculate the dHo of the Synthesis reaction using the values from the table in Appendix 2. Show your work. (2 points)

8. If 4 moles of H2 is used in a balanced equation for the synthesis reaction, how many moles of water will be produced (without using the tables). Show your work. (1 point)

9. If 4 moles of H2 is used for the Synthesis reaction, calculate the enthalpy of the reaction without using the tables. Show your work. (1 point)

10. If 4 moles of H₂O is required to be produced, how many moles of H₂ and how many moles of O₂ will be required (without using tables). Show your work. (1 point).

11. If 1 mole of water is required to be produced, how many moles of H₂ and O₂ will be required (without using tables)? Show your work. (1 point)

12. If 6 moles of water is decomposed, how many moles of H₂ and O₂ will be formed? (1 point)

13. If 6 moles of water is decomposed, calculate the enthalpy of the reaction without using the values from the table available in Appendix 2 of your textbook. (2 points)

Michael Farday weighs out 3.12 g. of salicylic acid in a 100 mL flask and adds 1.89 mL of acetic anhydride (density = 1.080 g/mL). Determine the maximum (theoretical) number of grams of acetylsalicylic acid he can prepare. If Mr. Faraday obtained 3.38 g. of Aspirin, calculate the % yield. Briefly, explain why he might have obtained this amount of product.

Determine the oxidation number of iodine in each of the following compounds. Be sure to enter your answer as X+ or X-

(a)NaI

(b)I2

(c)IO2

(d)I2O7

(e)KIO4

(f)Ca(IO)2

Assuming complete disassociation of electrolytes which of these aqueous solutions has the LOWEST freezing point (reminder 1 molal=1 mol kg-1) 0.15 molal KCl 0.20 molal methanol 0.40 molal methanol 0.10 molal K2O 0.10 molal KCln

Determine whether or not Hg2Br2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part B

This question will be shown after you complete previous question(s).

Part C

Determine whether or not Mg(OH)2 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part D

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Part E

Determine whether or not CaCO3 will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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Part F

This question will be shown after you complete previous question(s).

Part G

Determine whether or not AgI will be more soluble in acidic solution than in pure water.

Determine whether or not  will be more soluble in acidic solution than in pure water.

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A 23.33-mL solution containing 1.718 g Mg(NO₃)₂ is mixed with a 30.50-mL solution containing 1.467 g NaOH. Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive. If a species fully precipitates, type 0.

a.) ______ M Mg²⁺

b.) ______ M NO₃^-

c.) ______ M Na⁺

d.) ______ M OH^-

Use Avagadros number to calculate the number of molecules of H2S, the number of atoms of H, and the number of atoms of S, in 5.25 moles of H2S. Show all work and keep track of units and significant figures.

Why can the values of the apparant rate constant, Kapp, differ but the values of the true rate constant, k, be indentical in a reaction. An example of a reaction this can happen in is CH3COOCH3 + H20 → CH3OH + CH3COOH

What will the final temperature of 400 mL sample of water at 39.2°C be if 36,555 J of heat were added.

a.88.1°C

b.58.2°C

c.77.0°C

d.61.0°C

How much heat is produced when 6.26g of zinc metal reacts with oxygen gas under standard conditions? Use standard enthalpies of formation provided in your textbook.

a. 35.5 kj

b.267 kj

c.1021 kj

68.7 kj

Ethanol, C2H5OH, is used as a primary fuel for motor vehicles in some countries like brazil,The balanced chemical equation for the combustion reaction is

C2H5OH(l) + O2(g)-------- CO2(g) + H2O(g)

The density of the ethanol is 0.7893g/mL .Determine the enthalpy of combustion of exactly 2L of ethanol.

a. -3.31 x 10^4 kj

b.-4.68 x 104

c.-1.11 x 104 kj

d.1.69 x 10^4 kj

Determine the [OH?] of a solution that is 0.115M in CO32-.

The kb value for CO32- is 2.1e-4.

Determine the pH and pOH of a solution that is .115 M in CO32-

Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture.

pKa1 = 1.30

pKa2 = 6.70

Calculate the pH for each of the following points in the titration of 50.0 mL of a 2.7 M H3PO3(aq) with 2.7 M KOH(aq).

A) before addition of any KOH

B) after addition of 25.0 mL of KOH

C) after addition of 50.0 mL of KOH

D) after addition of 75.0 mL of KOH

E) after addition of 100.0 mL of KOH

Describe the acidity and pKa of hydrogen atoms that are bonded to carbon atoms adjacent to alkenes, as compared to hydrogen atoms bonded to tertiary alkanes. What happens to leaving groups that are found in the same adjacent position?

3. Ion exchange chromatography

a) how can the texhnique be used for qualitative and quantitative purposes

b) what are the major advantages and limitations of the technique

c) describe the nature of the signal (what is actually being detected)

What are the intermolecular forces involved with CO2?

A system contains a 0.1 molar solution of NaCl and a 0.01 M solution of NaCl separated by an oherise impermeable membrane hat contains a special sodium-conducting pore called an ionophore. The 0.1M solution is inside the membane and the 0.01 Molar solution is outsie the membrane. This ionophore allows free diffusion of the Na+ ions, but not Cl- ions. T=300K, R= 8.31 J/K/mol, F= 96500 J/mol/volt...

a) what is the total chemical potential difference, that includes concentration dependent potential and electrical potential, in Joules/mol (outside minus inside) for the sodium ions?

b) considering that chemical potential can have both a concentration dependent component and an electrical component, what is the electrical potential, in volts, of the inside of the memebrane with respect to the outside?

c) what is the chemical potential difference in Joule/mol (inside minus outside) for the chloride ions.