What are the clear differences in reduction of [Co(NH3)5MoO4] + and [Co(NH3)5CrO4] + by L-ascorbic acid? Would you expect L-ascorbic acid to reduce the Co(III), Cr(VI), and Mo(VI) metal centers when you discuss this interesting chemistry?

In the reaction of nitrogen gas with oxygen gas to produce nitrogen oxide. What is the effect of adding more nitrogen gas to the initial reaction mixture? N2+O2-2NO. A) the equilibrium shifts to produce more N2 b) the temperature of the reaction is raised c) extra catalyst is required to reach equilibrium d) the equilibrium shifts to produce more NO e) the equilibrium Is not effected

(THIS IS A MIXTURE OF ALL OF THE FOLLOWING ACIDS AND BASES MIXED TOGETHER WHERE A COMBINED pH IS WHAT I AM LOOKING FOR)

1. I have 0.500 Liters of water. To that 0.500 Liters, I add the following: a. 0.100 moles HCl b. 0.100 moles HOAc c. 0.100 moles NH4Cl d. 0.100 moles HF e. 0.050 moles NaOH f. 0.050 moles NaOAc g. 0.050 moles Mg(OH)2 What is the pH of the resulting mixture of everything?

Dissociation constants of acids: HOAc Ka=1.78x10-5 H2SO4 Ka1=1x107 Ka2=1.0x10-2 HCNO Ka=2x10-4 H2CO3 Ka1=4.3x10-7 Ka2=5.6x10-11 H2O Ka=1.0x10-14 HIO Ka=2.3x10-11 HNO2 Ka=4.5x10-4 HIO3 Ka = 1.7x10-4 HCl Ka=1x108 HNO3 Ka=1x106 HF Ka = 3.5x10-4 H2C2O4 Ka1 = 6.0x10-2 Ka2 = 6.1x10-5

Dissociation constants of bases: NH3 Kb=1.76x10-5 CH3NH2 Kb=4.4x10-4 NH2OH Kb=1.1x10-8 (CH3)3N Kb=6.5x10-5 C5H5N Kb=1.8x10-9 Mg(OH)2 Kb = 1 x106 NaOH Kb = 1x108

Raoult's Law describes a simple relationship between the vapor pressure of an ideal solution and the vapor pressure of pure solvent. Non-ideal solutions, however, show deviation from this ideal behavior. Solutions with vapor pressures lower than predicted (negative deviation) are the result of?

Mass of flask and foil(g) - 64.5297g

Mass of flask, foil and condensed vapor - 64.9787g

Temperature of boiling water bath - 101.2 C

Volume of flask (mL) - 153.0

Barometric pressure - 762.4 mmHg

Room temp - 23 C

Vapor pressure at room temperature - 100 mmHg

Calculate:
1. Uncorrected mass of condensed vapor(g)

2. Corrected density of air(g/L)

3. Average volume of flask (L)

4. Initial mass of air in flask (g)

5. Final partial pressure of air in flask (mmHg)

6.FInal mass of air in flask (g)

7.Mass of air lost (g)
8. Corrected mass of condensed vapor(g)
9. Molecuular weight (g/mol)

Calculate the percent ionization of 8.0

Why does the antifreeze ethylene glycol, HO-CH2-CH2-OH, molar mass 62.07 g/mol, have a much higher higher boiling point (197.6°C) than propanol (97.4°C), CH3-CH3-CH2-OH, molar mass 60.09 g/mol, even though they have similar molar masses?

As a technician in a large pharmaceutical research firm, you need to produce 450. mL of a potassium dihydrogen phosphate buffer solution of pH = 6.91. The pKa of H2PO4− is 7.21. You have the following supplies: 2.00 L of 1.00 M KH2PO4 stock solution, 1.50 L of 1.00 M K2HPO4 stock solution, and a carboy of pure distilled H2O. How much 1.00 M KH2PO4 will you need to make this solution? (Assume additive volumes.)

What is the Henry's law constant for CO2 at 20∘C?

Express your answer to three significant figures and include the appropriate units.

What pressure is required to achieve a CO2 concentration of 9.40×10⁻² M at 20∘C?

Express your answer to three significant figures and include the appropriate units.

At 1 atm, how many moles of CO2 are released by raising the temperature of 1 liter of water from 20∘C to 25∘C?

Express your answer to four decimal places and include the appropriate units.

The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. \(4NH_{3}(g)+5O_{2} --> 4NO+6H_{2}O(g)\) What is the maximum mass of H2O that can be produced by combining 72.0 g of each reactant?

Calculate the amount of sodium oxalate needed to react with 1.5 ml of 0.02M of KMNO4 solution.

The solutions at the two Pb electrodes of a concentration cell were prepared as follows:

Cell A: A mixture of 1.00 mL of 0.0500 M Pb(NO₃)₂ with 4.00 mL of 0.0500 M KX (the soluble potassium salt of an unspecified monovalent ion X^-).
Some PbX₂(s) precipitates.

Cell B: 5.00 mL of 0.0500 M Pb(NO₃)₂.

The cell potential was measured to be 0.05600 V at 25 °C.

1.By use of the Nernst equation, determine the concentration (M) of Pb²⁺ in the solution of Cell A.

2.In Cell A, how many moles of X^- have reacted with Pb²⁺?

3.What is the concentration (M) of X^- in the solution of cell A.

4.Calculate K_sp of PbX₂.

Ag⁺ + Cl^- ↔ AgCl(s)

1.004 g of an impure mixture containing Cl- was dissolved to 100.0 mL. 10.00 mL of this solution required 22.97 mL of 0.05274 M AgNO3 to reach end point. What is the weight percent of Cl- in the unknown solid?

consider the isoelectronic ions Cl- and K+. Which ion is smaller?

ssuming the core electrons contribute 1.00 and valence electrons contribute nothing to the screening constant, S, calculate Zeff for these two ions.

Repeat this calculation using slater's rules to estimate the screening constant, S. For esoelectronic ions how are effective nuclear charge and ionic radius related?