Substance H has maximum absorbance at 550 nm; Substance M has maximum absorbance at
650 nm. A standard solution of H has a concentration 74.2 ppm and an absorbance of 0.972 at
500 nm and an absorbance of 0.276 at 650 nm. A standard solution of M has a concentration
of 35.9 ppm and an absorbance of 0.102 at 500 nm and of 0.564 at 650 nm. A sample solution
that is a mixture of H and M has an absorbance of 0.756 at 500 nm and 0.818 at 650 nm. What
is the concentration of H and of M in the sample solution?

Each of the isomers can be formed, but 4-methylcyclohexene is the major product formed. Why?

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation

MnO2(s)+4HCl(aq)⟶MnCl2(aq)+2H2O(l)+Cl2(g)

How much MnO2(s) should be added to excess HCl(aq) to obtain 155 mL Cl2(g) at 25 °C and 725 Torr?

Compare and contrast scanning tunneling microscopy (STM) and atomic force microscopy (AFM)? List at least two advantages and two disadvantages for both methods. Please reference at least one source in your discussion. (It may be a textbook.)

The vinegar sold in the grocery stores is described as 5.0%(V/V) acetic acid?

What is the molarity of this solution (density of 100% acetic acid is 1.05 g/mL)?

What is the mass % of acetic acid in this solution (density of vinegar is 1.01 g/mL)?

What is the mole fraction of acetic acid in this solution?

What is the molality of this solution?

Please explain as you solve

which of following statement is true of nuclear fusion

a. the mass of the products is greater than the mass of the reactant, and energy is absorbed

b. the mass of the products is greater than the mass of the reactants, and energy is released

c. the mass of the products is less than the mass of the reactants and energy absorbed

d. the mass of the products is less than the mass of the reactants, and energy is released.

A 5.00 mL volume of a 0.60 M solution of phosphoric acid, H3PO4(aq), reacts with 45.00 mL of 0.25 M NaOH(aq) according to the reaction below. The temperature of the solution rises from 26.0 °C to 28.0 °C. Assume the volumes of the solutions are additive, the density of the final solution is 1.10 g mL–1 , the heat capacity of the solution is the same as water and the water produced by the reaction does not affect the volume of the resulting solution. Calculate the molar enthalpy change for the reaction.

H3PO4(aq) + 3 NaOH(aq) ® Na3PO4(aq) + 3 H2O(l) Hrxn = ?

Compare the methods of capillary electrophoresis and high performance liquid chromatography HPLC. For each method, give an example of when it would be more advantageous than the other one.

***Please show ALL work and explain***

If 2.000 g NaHCO3 and 2.0 mL HCl (density = 1.18 g/mL) are reacted to yield 1.100 g NaCl, what is the theoreticaal and percent yield of this reaction?

Describe clearly how you would apply the concepts of pH control of natural waters and redox chemistry to precipitate or remove dissolved metals from acid mine water. Explain how pH and redox potential can be manipulated to remove different metals from solution. The metals may include: iron, copper, lead, zinc, arsenic, chromium

what period three element has the following ionization energies? (all in kj/mol)
IE1=1012, IE2=1900, IE3=2910, IE4=4960, IE5=6270, IE6=22,200

explain whether it is possible to determine the approximate concentration if a solution of that sample has an absorbance of 0.62

An aqueous solution is made by dissolving 21.2 grams of ammonium phosphate in 323 grams of water.

The molality of ammonium phosphate in the solution is ? m.

In the laboratory you are asked to make a 0.150 m potassium sulfide solution using 15.7 grams of potassium sulfide.  

How much water should you add?  
grams

If 20.9 grams of an aqueous solution of ammonium phosphate, (NH₄)₃PO₄, contains 3.33 grams of ammonium phosphate, what is the percentage by mass of ammonium phosphate in the solution?

% (NH₄)₃PO₄

How many grams of KF are there in 195 grams of an aqueous solution that is 10.8 % by weight KF.

g KF

Using the equation:      2 NO     +     O2       à    2 NO₂

Determine the limiting reactant if given 1.0 mol NO and 1.0 mol O₂

Determine the limiting reactant if given 4.2 mol NO and 2.0 mol O₂

Determine the limiting reactant if given 10.0 grams NO and 10.0 grams O₂

Identify the species that is oxidized and the species that is reduced in each of the reactions below:

Fe     +     Cu²⁺     à Fe²⁺     +      Cu

Mg     +    Fe²⁺     à    Mg²⁺     +    Fe