A student ran the following reaction in the laboratory at 610 K:

CO(g) + Cl2(g) COCl2(g)

When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.72×10-2 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

2.A student ran the following reaction in the laboratory at 546 K:

COCl2(g) CO(g) + Cl2(g)  

When she introduced 0.854 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 0.817 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

3. Consider the following reaction:

COCl2(g) CO(g) + Cl2(g)

If 6.56×10-3 moles of COCl2, 0.377 moles of CO, and 0.372 moles of Cl2 are at equilibrium in a 16.9 L container at 772 K, the value of the equilibrium constant, Kp, is

What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide to 5.00 L of 0.200 M ammonia? Ka of ammonium is 5.8 x 10^-10

2) What is the pH of the buffer after 90.0mL of 2.00 M HCl are added?

3) What is the pH of the buffer if 15.00 g of NaOH is added to the original buffer solution?

40.00 mL of a 0.1000 M carbonic acid (H₂CO₃) was titrated with 0.2000 M sodium hydroxide.

carbonic acid pka1:6.35 pka2:10.33

1.Calculate the volume of sodium hydroxide required to reach the first equivalence point.

2.Calculate the volume of sodium hydroxide required to reach the second equivalence point.

3.Write the balanced acid-base reaction and calculate the pH before the addition of sodium hydroxide.

4.Write the balanced acid-base reaction and calculate the pH after the addition of 12.00 mL of sodium hydroxide

5.Write the balanced acid-base reaction and calculate the pH after the addition of 20.00 mL of sodium hydroxide

6. Write the balanced acid-base reaction and calculate the pH after the addition of 30.00 mL of sodium hydroxide

7.Write the balanced acid-base reaction and calculate the pH after the addition of 40.00 mL of sodium hydroxide

8.Write the balanced acid-base reaction (paper only) and calculate the pH after the addition of 44.00 mL of sodium hydroxide

to a 100.0 mL volumetric flask are added 1.00 mL volumes of three solutions: .0100 M AgNO3, .205 M NaBr, and .100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigerously. What mass of AgBr would precipitate from this mixture? Hint: The Ksp of AgBr is 5.4 x 10-13 and the Kf of Ag(CN)2- is 1.0 x 10^21

For the reaction shown below, the initial concentrations for reactants and products are as follows: [A] = 0.27 M, [B] = 0.0640 M, [C] = 0.0134 M, and [D] = 1.47 M. If the equilibrium constant for the reaction is K_C = 0.802, which direction does the reaction have to shift to reach equilibrium?

A + 3B ⇌ 2C + 3D

Enter 1 if it shifts left, 2 if it shifts right, or 3 if it's already at equilibrium.

A sample of carbonic acid (0.125 L, 0.199 M, pK_a1 = 6.35, pK_a2 = 10.33) was titrated with 1.75 M NaOH. Calculate the pH at the following points:

Before the titration.

At the 1st midpoint.

why are thermoset plastics not affected by solvents to the same extent as thermoplastics?

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react.

PCl_3(g) + Cl_2(g) ⇌ PCl_5(g)

The equilibrium constant for the reaction is K_C = 37.8 at 110 °C. If 0.887 mol of phosphorus trichloride is added to 0.550 mol of chlorine in a 1.02-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride?

Report your answer to THREE significant figures.

500 lbm/min hydrocarbon feed is pumped into the feed point halfway to the top of a distillation tower. The tower feed point is 40.0 feet above holding tank for the hydrocarbon. The pressure in the holding tank is 25.0 psia. The pressure in the tower at the feed point is 85.0 psia. Assume the energy lost due to friction is negligible. There is no significant change in velocity. The hydrocarbon density is 55.0 lbm/ft 3 . Calculate the pump power required in hp and watts.

A mixture of gases is at equilibrium:

4 NO (g) → 2 N2O (g) + O2 (g) ∆H = -199.5 kJ

(a) Does the equilibrium shift to the left or to the right when some O2 (g) is removed from the reaction mixture?

(b) Does the equilibrium shift to the left or to the right when some NO (g) is added to the reaction mixture?

c) In which direction does the equilibrium shift as the temperature is lowered?

(d) In which direction does the equilibrium shift as pressure is applied to the system?

A volume of 13.96 mL of 0.1060 M NaOH solution was used to titrate a 0.618 g sample of unknown containing HC₇H₅O₃.

What is the molecular mass of HC₇H₅O₃? (report answers to 4 or 5 significant figures) 1.3812×10² g/mol

What is the percent by mass of HC₇H₅O₃ in the unknown?

In this problem what mass of sample in grams would be needed to deliver about 23.40 mL in the next trial?

In the second trial above, exactly 1.032 g was transferred into a flask to be titrated. If the initial buret reading is 0.10 mL, predict what the final buret reading be. ?

how do i find ksp

In Southern Ontario, during freezing weather CaCl2 is spread on icy highways to melt the ice. Calculate the freezing point lowering and freezing point of a solution containing 250 g of CaCl2 in 500.0 g of water.

Fe(II) can be precipitated from a slightly basic aqueous solution by bubbling oxygen through the solution, wheich converts Fe(II) to insoluble Fe(III):

4Fe(OH)⁺(aq)+4OH^-(aq)+O₂(g)+2H₂O(l) arrow 4Fe(OH)₃(s)

How many grams of O₂ are consumed to precipitate all of the iron in 5.0 x 10¹ mL of 0.065 M Fe(II)?

Please explain!

1.a.) The heat of hydrogenation of cyclohexane is -120kJ/mol. The heat of hydrogenation benzene is -208kJ/mol. Is the heat of hydrogenation of benzene more or less than you would expect

1.b.) This is the value different from the expected?