When ammonia is added to a solution that has Cu(OH)2(s) precipitate in it, the precipitate dissolves. Use Le Châtelier’s principle to explain this.

1. For the following reaction, 4.68 grams of butane (C₄H₁₀) are allowed to react with 20.3 grams of oxygen gas .

butane (C₄H₁₀)(g) + oxygen(g) ---> carbon dioxide(g) + water(g)

What is the maximum amount of carbon dioxide that can be formed?

What is the FORMULA for the limiting reagent?

What amount of the excess reagent remains after the reaction is complete?

2. For the following reaction, 24.8 grams of diphosphorus pentoxide are allowed to react with 12.6 grams of water .

diphosphorus pentoxide(s) + water(l) ---> phosphoric acid(aq)

What is the maximum mass of phosphoric acid that can be formed?

What is the FORMULA for the limiting reagent?

What mass of the excess reagent remains after the reaction is complete?

3. For the following reaction, 46.0 grams of iron are allowed to react with 18.4 grams of oxygen gas .

iron(s) + oxygen(g) ---> iron(III) oxide(s)

What is the maximum mass of iron(III) oxide that can be formed?

What is the FORMULA for the limiting reagent?

What mass of the excess reagent remains after the reaction is complete?

How do you use the Rydberg equation to determine the color of a flame test for an element. For example how do we know that potassium gives off a violet color during a flame test using the Rydberg equation?

Calculate the molarity (M) of 150.6 g of H2SO4 in 1.290 L of solution.

Please explain the affects that concentration of monomer can have on typical a radical polymerization

What is the equilibrium concentration of Ni^2+ (aq) in the solution. If one millimole of Ni(NO3)2 dissolves in 220.0 mL of a solution that is 0.300 M in ammonia?

mass of Na2S2O3 is 1.220g

titration of bleach with Na2S2O3 solution:

trial 1: total volume used 66mL

trial 2: total volume used 73.8mL

Density of Bleach 1.074 kg/L

a) find the moles of Na2S2O3 used to titrate the bleach solution

b)find the moles of I2 formed by reaction with bleach

c) find the molarity of OCl- present in the bleach solution

d) find the grams of NaOCl present in the bleach

e) find the percent NaOCl present in the bleach

What is the molarity of a solution containing 13.7 grams of NH3 in 1.55 liters of solution?

Calculate the pH of a 0.100 M sodium benzoate, NaC6H5CO2, solution. The Ka of acetic acid is 6.3 x 10-5

The vapor pressure of benzene is 73.03 mm Hg at 25 °C. A nonvolatile, nonelectrolyte that dissolves in benzene is cholesterol.  

Calculate the vapor pressure of the solution at 25 °C when 5.507 grams of cholesterol, C₂₇H₄₆O (386.6 g/mol), are dissolved in 205.6 grams of benzene.

benzene = C₆H₆ = 78.12 g/mol.

VP(solution) = ____ mm Hg

Fill out table and show all calculations

Final             Volume of              Volume of               Volume of       Final volume (uL)

[PNPP] mM   0.5mM PNPP(ul)   0.2M Tris-HCl(ul)   enzyme (uL)

0.01                                                                            100                        1500

0.02                                                                             100                       1500

0.04                                                                             100                         1500

0.06                                                                            100                            1500

0.08                                                                            100                              1500

0.1                                                                           100                             1500

0.2                                                                              100                               1500

0.3                                                                           100                               1500

0.4                                                                             100                                1500

1.

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 = 35.9 at 119 °C. If 0.489 mol of phosphorus trichloride is added to 0.802 mol of chlorine in a 1.08-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride?

2.

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures.

N_2(g) + O_2(g) ⇌ 2 NO_(g)

The equilibrium constant for the reaction is K_P = 0.242 at 1200 °C. If a container is charged with 0.243 atm of nitrogen and 0.101 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

3.

Consider reaction (1) shown below with it's associated equilibrium constant. What is the equilibrium constant for reaction (2)?

Report your answer to THREE significant figures.

   (1)     A + 3 B ⇌ 2 C , K = 0.259

   (2)    2 A + 6 B ⇌ 4 C , K = ??

The pressure-based equilibrium constant for the reaction shown below is K_P = 3.575 at 443 °C. What is the value of K_C at this temperature?

2 NO_(g) + O_2(g) ⇌ 2 NO_2(g)

If you have a 4.00 mg sample of a radionuclide known as Q-234, calculate the mass that will remain after 5.00 years given that the half life of Q-234 is 2.5 years.