CHM 114 Midterm: Exam 1

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turquoisegnu128

31 Jan 2019

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P(s) + 3/2 h2(g) + 2o2(g) h3po4(l) Sample exam 1: thermodynamics is applied to learn about a reaction(cid:146)s, pathway, mechanism, stoichiometry, rate, spontaneity, in aqueous solution, iodine reacts with acetone as represented by the following equation: I2 + ch3coch3 ch3coch2i + h+ + i- O(g) + o3(g) 2o2(g: o(g, o3(g, o2(g, o2(g) and o(g, o3(g) and o2(g) (fast) (slow, a first-order reaction has a rate constant of 0. 021 s-1. The half-life for this reaction is: c, 48 s, 0. 030 s, 33 s, 0. 021 s, not enough data is provided for this calculation. Sample exam 1: hypochlorite ion oxidizes iodide ion in aqueous solution as represented by the equation: The rate of formation of hypoiodite ion (oi-) is given by the rate law. The overall reaction order is: 0, 1, 2, 3, k[i-][ocl-]/[oh-, the following data were measured for the reaction: Sample exam 1: consider the following energy diagram for a chemical reaction. Sample exam 1: consider the following reaction:

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Using the following information, calculate the number of moles of HCl, Moles of Borate, Concentration of Borate, Ksp, Average Ksp, ÎG (kJ/mol), ÎH (kJ/mol), and ÎS (J/mol*K):

Na₂B₄O₇ â¢ 10H₂O(s) -><- 2Na⁺(aq) + B₄O₅(OH)₄^2â(aq) + 8H₂O(l)

Titration: B₄O₅(OH)₄^2-(aq) + 2HCl(aq) + 3H₂O(l) â 4 B(OH)₃(aq) + 2 Cl^â (aq)

Molar Mass of B: 10.81g/mol, Molar Mass of O: 16.00g/mol, Molar Mass of H: 1.008g/mol, Molar Mass of Cl: 35.45g/mol

K = [Na⁺]² [B₄O₅(OH)₄^2-]

Ksp = 4 [B₄O₅(OH)₄^2-]³

ÎG = âRT ln Ksp

ÎG = ÎH â TÎS

âRT ln Ksp = = ÎH â TÎS

a)Titration 1: Temperature: 28.0 degrees C, Concentration of HCl: 0.251 M, Volume of Borax solution (mL): 5.00, Volume of HCl titrated: 2.00 mL

Please do not post the lab that this question comes from because it is hard for me to understand. Please show each individual step and use units along the way to the answer. Thanks!

Please answer the following questions AND SHOW WORK ifapplicable--I do not understand some of them! (750 value)

1. How many moles of chloride ions are present in 18.4g ofCaCl2?

2. Complete the follow reaction and identify the Bronstedbase:

NaOH (aq) + HCl (aq) ---> ________________

3. A candy bar contains 280 Calories, of which the fat contentaccounts for 120 Calories. What is the energy of the fat content,in kJ?

4. 25 kJ of heat is absorbed and 15 kJ of work is done on thesurroundings. What is /\U?

5. What is the change in internal energy in joules for a systemthat releases 154 J of heat and does 125 J of work on itssurroundings?

6. Ice packs, have lower temperatures when ammonium nitratedissolves in water--which of the following is true of thisreaction?

A. /\H<0, process is exothermic

B. /\H>0, process is exothermic

C. /\H<0, process is endothermic

D. /\H>0, process is endothermic

E. /\H=0, since cold packs are sealed

7. 2SO2 + O2 ----> 2SO3, /\H degrees rxn = -198kJ/mol, howmuch heat is evolved when 600 g of SO2 is burned?

8. Calculate /\H degree rxn for the following reaction:

2H2O2 ---> 2H2O +O2

*Given that /\H degree f [H2O] = -285.8 kJ/mol and /\H dgree f[H2O2] = 187.6 kJ/mol

9. For the following reaction, write the half-reactions, the netreaction, and identify the oxidizing agent:

H2SO4 + Cd(OH)2 ----> 2H2O + CdSO4

THANK YOU!

1. Calculate the standard change in free energy ?G? (kJ) at 298 K for the reaction C2H4(G)+3o2(G) --> 2CO2(G)+2H2O(G)

a -1310 b. +1180 c. -691 d. +1310 e. -1180

2. The value of E?cell for the reaction 2Cr3+(aq)+6Hg(l) --> 2Cr(s)+3Hg22+(aq) is 1.59 V. Calculate the ?G? (kJ) for the reaction.

a. -921 b. -153 c. -767 d. -460 e. -307

3. What is the value of the equilibrium constant for the cell reaction below at 25 deg C? E?cellÂ=0.61V 2Cr(s)+3Pb2+(aq) <---> 3Pb(s)+2Cr3+(aq)

a. 8.2*10^30 b. 6.7*10^61 c. 9.9*10^99 d. 4.1*10^20 e. 3.3*10^51

4. Which one of the following is not a redox reaction?

a. Na6FeCl8(s)+2Na(l) ---> 8NaCl(s)+Fe(s)

b. Al(OH)3 (aq)+3H+ ---> Al3+(aq)+3H2O(l)

c. CuCl2(aq)+Ni(s) ---> Cu(s)+NiCl2(aq)

d. C6H12O6(s)+6O2(g) ---> 6CO2+6H2O(l)

e. COÂ2(g)+H2(g) ---> CO(g)+ H2O(g)ÂÂÂÂÂÂÂÂ

5. A voltaic cell consists of a Zn/ZN2+ electrode and a Fe/Fe2+ electrode. If [ZN2+] = 0.005M and if [Fe2+] = .0500 M , what is Ecell?

a. .76 b. 0.25 c. 0.45 d. 0.31 e. 0.37

6. The formation constant for the reaction Ag+ (aq)+2NH3(aq) <----> Ag(NH3)2+(aq) is K=1.7*107 at 25 deg C. What is the ?G?(kJ/mol) at this temperature?

a. -23 b. -18 c. -3.5 d. -1.5 e. -41

7. Nitric oxide reacts with chlorine to form NOCL. What is the free energy (kJ) of the reaction at 277 deg C?

a. +144 b.. -41.0 c. -10.3 d. -22.2 e. +41.0

8. Estimate the boiling point (deg C) of phosphoric Acid.

H3PO4(s) <----> HÂ3PO4(l)

?H?f kJ/mol -1279 - -127.17

?G?f kJ/mol -1119 - 1123.6

?S?f J/(k mol) 110.5 - 150.8

a. 42 b. 181 c. 315 d. -92 e. 305

9. Calculate the equilibrium constant, K, for the following reaction at 25?C:

CH4(g)+2H2O(g) <---> Ã CO2(g)+4H2(g) ?G?= -113.6 kJ (please show ICE chart and explain process)

a. 8.2x1019 b. 0.58 c. 0.96 d. 1.4x10-46 e. 1.2x10-20

10. Which of the following results in a decrease in the entropy of the system?

a. O2(g), 300K --> O2(g), 400K b. H2O(s) --> H2O(l) c. N2(g) --> N2(aq) d. NH3(l) --> NH3(g)

e. 2H2O2(g) ---> 2H2O(g)+O2(g)

CHM 114 Midterm: Exam 1

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