1. Your stoichiometry reaction is C → 1/3 D

A. You know the reaction order is second order in C. What is the rate law for this reaction? (Remember it has three parts)

B. If the reaction rate is 0.150 M/s when the concentration of C is 0.800, what rate would you expect if the concentration of C is 0.400M?

C. What rate of formation of D would you expect for your answer in part B (using the rate for 0.400 M C)?

2. We now have three equations we can use to predict concentration of reactants if we know the reaction order. Define the following:

A) What is k?

B) What is [A]t?

C) What is [A]o

D) What is t?

E.) How would you calculate the amount of reactant used in the reaction (using variables above)?

F.) How would you calculate the amount of product made in a reaction (using variables above)?

A) The substance sulfur dioxide has the following properties:

A sample of sulfur dioxide at a pressure of 1.00 atm and a temperature of 253.5 K is cooled at constant pressure to a temperature of 192.3 K. Which of the following are true?

Choose all that apply

The solid initially present will vaporize.

The sample is initially a liquid.

The final state of the substance is a solid.

One or more phase changes will occur.

The final state of the substance is a liquid.

B) The substance xenon has the following properties:

A sample of xenon is initially at a pressure of 63.9 atm and a temperature of 178.0 K. The pressure on the sample is reduced to 0.370 atm at a constant temperature of 178.0 K. Which of the following are true?

Choose all that apply

The sample is initially a liquid.

The liquid initially present will solidify.

One or more phase changes will occur.

The final state of the substance is a solid.

The final state of the substance is a gas.

What volume of 0.0100 M KMnO₄ solution is required to oxidize 42.5 mL of 0.0190 M FeSO₄ in sulfuric acid solution?

What is the pH of a solution containing 0.12 mol/L of NH4Cl and 0.03 mol/L of NaOH (pka of NH4+/NH3 is 9.25)?

Predict the bond angles in the following molecules.

1. What is the fraction 3/260 in scientific notation to 3 significant figures?

2. Which statement is correct about element? A) sulfur is a good conductor of heat B) iron is a transition metal C) boron is metal D) copper is a poor conductor

3. If an element has a mass number of 14, and contains 8 neurons, what is it's atomic number? A)22 B)6 C)14 D)8

4. What term describes urine sample with a ph value of 5.5? A)balanced  B)alkaline C)neutral D) acidic

5. Which term means the substance in which the solute is dissolving into? A)Solution B)Solvent C)Suspension

6. What is the oxidation number of magnesium (ma) with any compound? A) +3 B )+1 C) +2 D) 0

7. What term best describe NaoH in this reaction? HCl+NaoH=NaCl+H20 . A) Gas B) Product C) Acid D) Reactant

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

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

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