Tennessee State University Chemistry Worksheet

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** I only have 1 Hour** 20 Questions

1. Le Chatelier’s Principle is about changes to chemical equilibrium. Using your datasheet from you virtual lab. Explain in your own words what is happening and why for each of the following reactions:

1. When acid is added to the cobalt chloride solution. 2. When water is added to previous mixture. 3. When acid and then silver nitrate is to the cobalt chloride solution.

Match the following reactions to the reaction type.

Question 2 options:

Decomposition

Precipitation

Neutralization

Reduction

Oxidation

CO2(g) + H2(g) <---- data-verified=“> CO(g) + H2O(g)

Mg(NO3)2(aq) + Na2CO3(aq) ----- data-verified=“>

MgCO3(s) + NaNO3(aq)

2HgO(s)→2Hg(l)+O2(g)

2 Fe(s) + 3 O2(g) ----- data-verified=“> 2 Fe2O3(s)

3Ca(OH)2 +2H3PO4 →

6H2O + Ca3(PO4)2

3. 2AlBr3 + 3K2SO4 → 6KBr + Al2(SO4)3

Using this balanced equation: Answer the following parts of this question. Must show your work to receive full or partial credit. The initial masses: AlBr3 = 7.145 g and K2SO4 = 6.839 g

Periodic Table: https://sciencenotes.org/wp-content/uploads/2018/08/NoNamePeriodicTable118.png

1. Calculate all the molar masses. 2. Identify the limiting reagent when focused on producing Al2(SO4)3 . 3. Calculate the theoretical yield for Al2(SO4)3 . 4. Calculate the percent yield if 3.952 g of Al2(SO4)3 was recovered.

4. Balance the following equation:

Enter a coefficients into each box. 1st coefficient corresponds with the 1st box. 2nd to 2nd box, etc.

___ As + ___NaOH → ___Na3AsO3 + ___H2


5. Balance the following equation:

Enter a coefficients into each box. 1st coefficient corresponds with the 1st box. 2nd to 2nd box, etc.

___C7H6O2 + ___O2 → ___CO2 + ___H2O


6. Write 5 different laboratory safety rules/practices that you must follow when performing an experiment. (2 points each – 10 points total)



7. How many grams of NaOH are there in 700 mL of a 0.225 M NaOH solution?

https://sciencenotes.org/wp-content/uploads/2018/08/NoNamePeriodicTable118.png

8. In a laboratory titration, 25.0 mL of NaOH is completely neutralized by 18.4 mL of 0.750 M HCl. What is the concentration of the NaOH solution?

9. Calculate the average deviation, in milliliters, for the following volumes.

45.1 mL, 0.0459 L, 44.8 cm^3, 4.56 cL

A.1.6 mL B.15.3 mL C.70.9 mL D.0.4 mL

10. In a laboratory titration, 25.0 mL of oxalic acid solution is completely oxidized by 0.500 M potassium permanganate. The initial volume of the buret is shown the picture where x = 13 mL. The final volume of potassium permanganate used is 35.0 mL. What is the concentration of the oxalic acid solution?

2KMnO4 + 5(COOH)2 + 3H2SO4 → 2MnSO4 + 10CO2 + 8H2O + K2SO4

11. 25 g of a compound is added to 500 mL of water if the freezing point of the resulting solution is 0.57 °C what is the molecular weight of the compound assume no molecular disassociation upon dissolution Kf equals 1.36 °C/m

A.238 g/mol B.60 g/mol C.119 g/mol D.90 g/mol

12. Using the chemical equation below: 0.175 M HCl is used to neutralize 0.150 Ba(OH)2. If 15 mL of base is used, what would be the volume acid need to neutralize the base?

2HCl(aq)+Ba(OH)2(aq)→BaCl2(aq)+2H2O(l)

A.12.8 mL B.25.7 mL C.15 mL D.19.2 mL

13. Calculate the % percent recovery the compounds. The initial mass of the mixture of compound A and B is 5.73 g. The compounds are separate using fractional crystallization. The mass of compound A was 3.48 g. The mass of compound B was 1.58 g

A.113% B.25.5% C.88.3% D.61.2%

14. Which of the following types of intermolecular forces provides the most accurate explanation for why noble gases can liquify?

A. Hydrogen Bonding B. Dipole-dipole interactions C.Ion-dipole interactions D.Dispersion Forces


15. What is the percent mass of chromium in K2Cr2O7?

A.40.2% B.38.1% C.26.6% D.35.4%


16. An unknown mixture is separated into compounds A and B. The % mass of compound A in the mixture is 61.78%. The mass of compound A and filter paper is 2.946 g. The mass of the filter paper is 0.371 g. Assuming 100% recovery of compounds, what is the initial mass of the mixture.

A.5.369 g B.4.768 g C.4.168 g D.4.368 g


17.

Above is the standard curve for the experiment. The following solution is prepared with 4.3 mL of 0.002 M KSCN, 10.5 mL of 0.002 M ferric nitrate and 6.2 mL of nitric acid. The absorbance is 0.53. Calculate the Kc value for the solution.

A.290.3 B.256.9 C.320.02 D.283.2


18. Given the following. What is the rate law for the reaction A + 2B → C

[A] [B] Rate (M/s)

0.1 0.02 0.01

0.2 0.02 0.04

0.1 0.01 0.005

A. Rate= k [A] B. Rate= k [A] [B]^2 C. Rate= k [A]^2[B] D. Rate= k [B] E. Rate= k [A][B]

19. Bonus: Watch this short video (5 points). Link are to the same video on different sites.

https://www.instagram.com/p/B-7pgdkjTkR/?utm_source=ig_web_copy_link or https://www.facebook.com/644199405752818/videos/516326362395321/

The iodine clock reactions in the initial beakers are changing quickly almost immediately one after the other. The last 3 beakers the reaction takes much longer. Explain what why this change in time for the last 3 beakers possibly happened and how it relates to the hydrogen peroxide concentration.

20. Bonus: Show your work to receive full or partial credit. (10 pts possible)

It’s January in Nashville and your local weather station just informed you that the temperature outside is 15.4°F. You estimate the amount of ice on your driveway to be approximately 30 kg. What is the minimum amount of sodium chloride in kilograms (kg) needed to lower the freezing point of the water so that the ice melts?

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