A galvanic cell consists of a iron electrode in 1 M Fe(NO3)2 and a copper electrode in 1 M Cu(NO3)2. What is the equilibrium constant for this reaction at 25oC? Enter you answer with 2 significant digits, using the syntax of "1.0x10(22)" for "1.0x1022"

  use the steady state approximation

2N2O5 (g) → 4NO2 (g) + O2 (g)

The mechanism is based on:

  N2O5 → NO2 + NO3    ka

  NO2 + NO3 → N2O5    k'a

  NO2 + NO3 → NO2 + O2 +NO   kb

  NO + N2O5 → NO2 + NO2 + NO2   kc

Why is it not possible to assign R or S to a compound if it is drawn such that the lowest-priority substituent is in the plane of the paper? What are some ways to handle this situation?

Workers in underwater diving suits necessarily breathe air at greater than normal pressure. If they are returned to the surface too rapidly, N2, dissolved in their blood at the previously higher pressure, comes out of solution and may cause emboli (gas bubbles in the bloodstream), bends, and decompression sickness. Blood at 37∘C and 1 bar pressure dissolves 1.3 mL of N2 gas (measured for pure N2 at 37∘C and 1 bar) in 100 mL of blood.

Part A

Calculate the volume of N2 likely to be liberated from the blood of a diver returned to 1 bar pressure after prolonged exposure to air pressure at 300 m of water (below the surface). The total blood volume of the average adult is 4.7 L; air contains 78 vol% N2.

Correct answer from the back of the txtbk is 1800 mL .....i just cant figure out how they got it. Thanks

Match each subtype of lipid listed on the right to all statements on the left that are appropriate to the lipid subtype.

Question 12 options:

Acetic Acid Serial Dilution

For part of the experiment, you will need to prepare 100 mL of 0.025 M CH3CO2H (acetic acid), starting from commercial “glacial” acetic acid, which has a concentration of 17.4 M. Devise a method using a two-step serial dilution to make 100 mL of 0.025 M acetic acid solution. The glassware available is a 100 mL volumetric flask, 50.00 mL volumetric flask, 1.00 mL volumetric pipet, and a 10 mL graduated pipet. For the first step, dilute 1.00 mL of glacial acetic acid to 50.00 mL to produce “Solution 1”. You will then use Solution 1 to make the 0.025 M concentration for step 2. Determine the volume of Solution 1 needed to make 100 mL of 0.025 M acetic acid.

0.025 M CH3CO2H

A. ___________

B.____________

Consider the reaction IO−4(aq)+2H2O(l)⇌H4IO−6(aq);Kc=3.5×10−2 If you start with 25.0 mL of a 0.905 M solution of NaIO4, and then dilute it with water to 500.0 mL, what is the concentration of H4IO−6 at equilibrium?

Under what conditions does nickel hydroxide, Ni (OH)₂, serve as a pseudocapacitive materials? Explain your reason.

The calcium carbonate in limestone reacts with HCl to produce a calcium chloride solution and carbon dioxide gas:

CaCO3(s)+2HCl(aq)→CaCl2(aq)+H2O(l)+CO2(g)

EXPRESS YOUR ANSWER WITH THE APPROPRIATE UNITS.

a) How many milliliters of 0.200 MHCl can react with 7.25 g CaCO3?

b) How many moles of CO2 form when 27.5 mL of 3.00 M HCl react?

c) What is the molarity of a HClsolution if the reaction of 205 mLof the HCl solution with excess CaCO3 produces 14.0 L of CO2gas at 725 mmHg and 18∘C?

Part A

In the PhET simulation, select the solute in the dropdown menu under the beaker. The ionic formula of the solute will display on the beaker. You can click the box adjacent to Show values to display the concentration of each solution. By setting the Solution Volume slider bar to the minimum and the Solute Amount slider bar to the top, you can maximize the number of saturated solutions you create.

List the following compounds in order of increasing concentration for their saturated solutions.

Rank from lowest to highest. To rank items as equivalent, overlap them. Gold(III) Chloride, Colbalt(II) Nitrate, Potassium Permaganate, Copper(II) Sulfate

Part C

A sucrose solution is prepared to a final concentration of 0.250 M . Convert this value into terms of g/L, molality, and mass % (molecular weight, MWsucrose = 342.296 g/mol ; density, ρsol′n = 1.02 g/mL ; mass of water, mwat = 934.4 g ). Note that the mass of solute is included in the density of the solution. Express the concentrations in grams per liter, molality, and mass percent to three significant figures separated by commas.

part D

Suppose 217.7 mg of PbCl2 was added to 15.0 mL of water in a flask, and the solution was allowed to reach equilibrium at 20.0 oC. Some solute remained at the bottom of the flask after equilibrium, and the solution was filtered to collect the remaining PbCl2, which had a mass of 60.8 mg . What is the solubility of PbCl2 (in g/L)?

Express the concentration in grams per liter to three significant figures.

What are the net ionic equations for...

- Magnesium and HCl

- Iron and HCl

- Copper and HCl

- Zinc and HCl

- Tin and HCl

- Lead and HCl

A ground state hydrogen atom absorbs a photon of light having a wavelength of 93.03 nm. It then gives off a photon having a wavelength of 93 nm. What is the final state of the hydrogen atom?

n_f= ?

Two identical flasks of the same volume are labeled A and B. Flask A contains NH₃(g) at   50_­­^oC and flask B contains HCl (g)_­ at 50^oC. KE=1/2 mv².

a) Which molecule is moving the most rapidly? Explain.

b) Give two ways you could increase the pressure in the flask containing the NH₃(g)

c) Do both molecules have the same kinetic energy? Justify your answer.

Chemical kinetics

For the reaction 2A + B → C + D + 2E, data for a run with [A]₀ = 800 mmol/L and [B]₀ = 2.00 mmol/L are

and data for a run with [A]₀ = 600 mmol/L and [B]₀ = 2.00 mmol/L are

Find the order with respect to each reactant (A and B) and the rate constant.

Consider the reaction H2 (g) + F2 (g) <-- --> 2HF (g) .At a certain temperature, 0.50 moles of hydrogen gas, 0.50 moles of fluorine gas and .25 moles of hydrogen fluoride gas are placed in a 5.0 L container. Determine if the gas is at equilibrium or not and predict the direction it will move in order to get to equilibrium. And, for the mixure of the gases, determine the final concentrations of each gas. (use an appropriate table). Then, determine the partial pressure of each gas at equilibrium and STP (use Dalton's Law). Standard Pressure is 1.00 atm.