1) Calculate the amount of energy (in kJ) necessary to convert 357 g of liquid water from 0*C to water vapor at 172*C. The molar heat of vaporization of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g*C, and for steam is 1.99 J/g*C.

2) The vapor pressure of ethanol is 1.00 x 10^2 mmHg at 34.90*C. What is its vapor pressure at 54.83*C? (deltaHvap for ethanol is 39.3 kJ/mol)

3) The vapor pressure of a liquid doubles when the temperature is raised from 85*C to 96*C. At what temperature will the vapor pressure be seven times the value at 85*C?

A 0.249g pellet of potassium hydroxide, KOH, is added to 64.0g water in a Styrofoam coffee cup. The water temperature rises from 23.5 to 24.4 ?C. [Assume that the specific heat of dilute KOH(aq)is the same as that of water.] What is the approximate heat of solution of KOH, expressed as kilojoules per mole of KOH?

Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following reactions. Answers must be in Kj.

Part A N2O4(g)→2NO2(g) Express your answer using two significant figures.

Part B NH4Cl(s)→HCl(g)+NH3(g) Express your answer using three significant figures.

Part C 3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g) Express your answer using three significant figures.

Part D N2(g)+3H2(g)→2NH3(g) Express your answer using three significant figures.

Part E How do the values of ΔG∘ calculated this way compare to those calculated from ΔH∘ and ΔS∘? Which of the two methods could be used to determine how ΔG∘ changes with temperature? Essay answers are limited to about 500 words (3800 characters maximum, including spaces). 3800 characters maximum.

Ringer's lactate, a solution containing several different salts, is often administered intravenously for the initial treatment of trauma patients. One liter of Ringer's lactate continas 0.102 mole of sodium chloride, 4.0 × 10^-3 mole of potassium chloride, 1.5 × 10^-3 mole of calcium chloride, and 2.8 × 10^-2 mole of sodium lactate. Determine the osmotic pressure (in atm) of the solution at normal body temperature (37^oC). Assume no ion pairing. (The formula of the lactate ion is HO-CH(CH₃)-COO^-.)

while transferring the weighed salt to the test tube during the experiment, a student spilled some.Will this salt loss result in calculated salt solubilities that are too high, too low, or unchaged? briefly explain.

Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following reactions.

NOBr(g)→NO(g)+1/2Br2(l)

NH4I(s)→HI(g)+NH3(g)

3H2(g)+Fe2O3(s)→2Fe(s)+3H2O(g)

NO(g)+1/2O2(g)→NO2(g)

Chemical Equilibrium gives us a snapshot of the possible interactions of potential chemical interaction of reacted or of partially reacted components of chemical. Many of our problems were hypothetical or postulated results, which (if known) give us insight into possibilities – discuss how knowing this helps us to know which reactions are most important and how this relates to utilization of fuel in combustion or assessing hypothetical pollutants at a snap shot in time.

Friedel-Crafts Alkylation is a special type of EAS reaction. The reaction involves the use of highly caustic and dangerous chemicals. Why are these conditions necessary? What conditions would be required if these chemicals were not used?

Calculate the pH of the solution that results from each of the following mixtures

A.) 150.0mL of 0.23M  HF with 225.0mL of 0.32M  NaF

B.) 185.0mL of 0.12M C2H5NH2 with 285.0mL of 0.22M C2H5NH3Cl

1. The equilibrium constant, K_c, for the following reaction is 9.52×10^-2at 350 K.

CH₄(g) + CCl₄(g) = 2 CH₂Cl₂(g)

Calculate the equilibrium concentrations of reactants and product when 0.300 moles of CH₄and 0.300 moles of CCl₄are introduced into a 1.00 L vessel at 350 K.

2. 2HI(g) =H₂(g) + I₂(g)

If 1.87 moles of HI, 0.335 moles of H₂, and 0.211 moles of I₂ are at equilibrium in a 15.6 L container at 748 K, the value of the equilibrium constant, K_p, is ?

3. The equilibrium constant, K_p, for the following reaction is 2.01 at 500 K:

PCl₃(g) + Cl₂(g) =PCl₅(g)

Calculate the equilibrium partial pressures of all species when PCl₃ and Cl₂, each at an intitial partial pressure of 0.829 atm, are introduced into an evacuated vessel at 500 K.

4. The equilibrium constant, K_p, for the following reaction is 1.80×10^-2 at 698 K:

2HI(g) = H₂(g) + I₂(g)

Calculate the equilibrium partial pressures of all species when HI(g) is introduced into an evacuated flask at a pressure of 1.29 atm at 698 K.

How much 5.60M NaOH must be added to 410.0 mL of a buffer that is 0.0205 Macetic acid and 0.0235 M sodium acetate to raise the pH to 5.75?

You would like to combine 3 kg of adipic acid with hexamethyl diamine to produce the polyamide nylon. Calculate a) the amount of ethylene glycol required. b) the amount of by product evolved and c) the amount of polyester produced. c) Differentiate between Nylon 6 and Nylon 6,6.

Calculate the coulombic energy difference between the Calcium-39 and Potassium-39 mirror pair. Also calculate the difference between the Nitrogen-13 and Carbon-13 pair. How do these compare to the energy obtained from mass balance principles?

1) Consider the following acid ionization constants:

Solutions of each are prepared in which the inital concentration of the acid is 0.1000 M. Which of the four solutions will have the lowest pH?

the answer is HA

Explain why it is HA

2) A certain first order reaction is 30% complete in 115 minutes. what is the half life ( t1/2) of the reaction?

a) 192 min

b) 223 min

c) 268 min

e) 66.2 min

ANSWER ALL QUESTIONS AND EXPLAIN WHY YOU CHOSE THE ANSWER

Theoretically, fractional distillation gives better separation than simpledistillation

.� Use mole ratios for early and late fractions from both simple and fractionaldistillations determined by GC analysis to calculate the volume and mole %composition of each. Present a single model of those calculations.

� Compare these mole % composition results to explain whether your experimentaldata supports this theory.

Data: Mole Ratio cyclohexane:touluene

Orginal mix: 1:1.05

early fractional simple : 1: 0.37

Late fractional simple : 1: 25

Early Fraction fractional: 1: 0.204

Late fraction fractional: 1: 194