Cl=8 F=22

(a) How many chlorine trifluoride molecules are formed in the reaction depicted above?

(b) How many chlorine molecules remain after the reaction has gone to completion?

(c) How many fluoride molecules remain after the reaction has gone to completion?

(d) Which is the limiting reactant in the reaction depicted above?

(e) If the reaction was carried out with 2.05 moles of chlorine gas and 4.46 moles of fluorine gas, how many moles of chlorine trifluoride would be produced?

(f) If the reaction was carried out with 2.05 g of chlorine gas and 4.46 g of fluorine gas, how many grams of chlorine trifluoride would be produced?

Titration of 50.0mL of 0.100M HX (Ka=1.5x10^-5) with 0.100M NaOH. Calculate the pH of:

- buffer formed at the addition of 12.5mL NaOH

- buffer formed at the addition of 25.0mL NaOH

- buffer formed at the addition of 37.5mL NaOH

- solution obtained at the endpoint

Please do the endpoint especially!

Sulfur hexafluoride and Sulfur tetrafluoride are two common halides of sulfur.

a) Draw their lewis dot structures and describe their molecular shapes including bond angles.

b) Write a balanced reaction for the synthesis of SF₆.

c) Describe in detail the differences in reactivity and chemistry of the observed by the two compounds.

d) Please describe in as much detail as possible, uses for SF₆.

A) A buffer solution contains 0.484 M KHCO₃ and 0.314 M K₂CO₃. Determine the pH change when 0.126 mol NaOH is added to 1.00 L of the buffer.

pH after addition − pH before addition = pH change =

B) A buffer solution contains 0.335 M NH₄Br and 0.313 M NH₃ (ammonia). Determine the pH change when 0.072 mol KOH is added to 1.00 L of the buffer.

pH after addition − pH before addition = pH change =

C) Determine the pH change when 0.086 mol HI is added to 1.00 L of a buffer solution that is 0.442 M in CH₃COOH and 0.368 M in CH₃COO^-.

pH after addition − pH before addition = pH change =

A) Consider how best to prepare one liter of a buffer solution with pH = 4.94 using one of the weak acid/conjugate base systems shown here.

How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?

grams potassium salt of weak acid =

grams potassium salt of conjugate base =

B) Design a buffer that has a pH of 3.75 using one of the weak acid/conjugate base systems shown below.

How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?

grams sodium salt of weak acid =  g

grams sodium salt of conjugate base =  g

C) Consider how to prepare a buffer solution with pH = 9.52 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.301-M solution of weak acid with 0.365 M potassium hydroxide.

How many L of the potassium hydroxide solution would have to be added to the acid solution of your choice?

Design a buffer that has a pH of 7.29 using one of the weak base/conjugate acid systems shown below.

D) How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?

grams chloride salt of conjugate acid =

grams weak base =

Calculate the pH of a 0.01 M solution of sodium benzoate.

A: Dissociation constant of benzoic acid.

B: Calculate the hydrolysis constant of sodium benzoate.

C: Calculate the pH of the 0.01 M solution.

Explain what is olefin metathesis? in one paragraph

The reaction of nitrogen gas with hydloric acid is as follows:

N_{2 (g)} + 6 HCl _(g)  

please calculate the

1.theoretical yield,

2.percent yield, and

3. overall percent yield from benzaldehyde.

my products weight was 2.137 g

experiment was "Isolation of Tetraphenylcyclopentadienone, then Recrystalization of Tetraphenylcyclopentadienone"

HERE IS MY PROTOCOL I FOLLOWED TO GET MASS OF 2.137 g

THIS IS ALL AVAILABLE INFORMATION!!!

Add 1.5 g benzil, 1.5 g dibenzyl ketone, and 12 mL absolute ethanol to a 50-mL round-bottom flask. Place a magnetic stir bar in the flask. Attach a condenser, having lightly greased the joint. Stir and heat the mixture at 70ºC (with the condenser running) until the solids dissolve. Then raise the temperature to 80ºC with continued stirring. Using a 9" Pasteur pipette, add dropwise 2.25 mL of ethanolic potassium hydroxide solution through the condenser into the flask; make an effort to prevent any drops from contacting the condenser walls (each drop should fall directly into the reaction mixture). The mixture will immediately turn a dark purple. Once you have added the potassium hydroxide, raise the temperature to about 85ºC. Stir the mixture at this temperature for 15 minutes.

Isolation of Tetraphenylcyclopentadienone

At the end of the heating period, remove the flask from the heat and allow it to cool to room temperature. Then place the flask in an ice-water bath for 5 minutes to complete the crystallization of the product. Collect the deep purple crystals on a Büchner funnel by vacuum filtration. Wash the crystals with 3 4-mL portions of ice-cold 95% ethanol; this wash solvent should be used to transfer crystals from the round-bottom flask to the Büchner funnel if they do not all come out when the mixture is initially poured into the funnel. After air-drying the crystals for a few minutes, complete the drying in a 100ºC-oven for a few minutes.

Recrystallizing Tetraphenylcyclopentadienone

Recrystallize your tetraphenylcyclopentadienone from a 1:1 mixture of 95% ethanol and toluene; approximately 24 mL of this solvent mixture will be required per gram of tetraphenylcyclopentadienone, but remember to only add the minimum boiling solvent necessary to dissolve the solute. Recover the crystals by vacuum filtration (as above) and redetermine the melting point.

Weigh the dried product and calculate the percent yield. Also calculate the overall percent yield from benzaldehyde. Determine the melting point. If the melting point is not within 2ºC of the literature value, you should recrystallize your product (see below).

Al(OH)3(s) + HCl(aq) --> AlCl3(aq) + H2O(I) a) balance the equation b)calculate the number of grams s of HCl that can reacct with 0.500 g of Al(OH)3. c) calculate the number of AlCl3 and the number of grams of H2O formed when 0.500g of Al(OH)3 reacts. d) show that your calculations from parts b and c are consistent with the law of conservation of mass.

A textile finishing process involves drying a fabric that has been treated with a volatile solvent. The drying process involves evaporation of solvent and removal of solvent vapor by air. The wet fabric entering the dryer contains 50% solvent. Solvent-free air enters the dryer at a rate of 8 kilograms per kilogram of dry (solvent-free) fabric. The drying process is 96% efficient (i.e., 96% of the entering solvent is removed from fabric).

(a) Calculate the percentage of solvent in the dried fabric by weight.

(b) What is the concentration of solvent in the dryer exhaust (in g/m³) if the exhaust is at 80 degrees C and 1 atm? The solvent has a molecular weight of 86.

Find the Gibbs free energy for G(T,P) for an ideal gas with constant c_v.

Aqueous hydrochloric acid HCl will react with solid sodium hydroxide NaOH to produce aqueous sodium chloride NaCl and liquid water H₂O . Suppose 28.1 g of hydrochloric acid is mixed with 17. g of sodium hydroxide. Calculate the maximum mass of sodium chloride that could be produced by the chemical reaction. Be sure your answer has the correct number of significant digits.

What are the principles of surface sorption by solid?