On the basis of your research, respond to the following:

Why and how does atomic nuclear decay take place? Explain.

What is the significance of atomic nuclear decay?

What is your analysis on the societal implications of using this process?

What is the purpose of sodium hydrosulfite addition? What is the purpose of potassium ferricyanide in the conversion of luminol to an excited state?

Calculate ?H (298 K) per gram of fuel units of kJ*g^-1 (exclude oxygen)

a.) H2(g) + 1/2 O2(g) = H2O(g)

b.) CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)

c.) CH3OH(l) + 3/2 O2(g) = CO2(g) + 2H2O(g)

d.) C6H14(g) + 9 1/2 O2(g) = 6CO2(g) + 7H2O(g)

A buffer contains 1.0 mol of CH3CO2H and 1.0 mol of CH3CO2- diluted with water to 1,0 L. How many moles of NaOH are required to increase the pH of the buffer to 5.10? pKa of CH2CO2H is 4.74

Can someone explain this step by step please!

Consider the distillation of ethanol (C2H5OH) and the combustion of ethanol . Use a bullet point list to compare and contrast the 2 processes. There should be at least 5 points of comparison

NH3 is a weak base (Kb = 1.8 × 10–5) and so the salt NH4Cl acts as a weak acid. What is the pH of a solution that is 0.011 M in NH4Cl at 25 °C?

Calculate the pH of a 0.19 M CH₃COOLi solution. (K_a for acetic acid = 1.8 × 10⁻⁵.)

Rank the following compounds in order of increasing strength of intermolecular attractions: H2O2, CF4, KF, and CHCl3

You have a 5 mL sample of a protein in 0.5 M NaCl. You place the protein/salt sample inside dialysis tubing (see below) and place the bag in a large beaker of distilled water. If your goal is to remove as much NaCl from the sample as possible, which would be more effective: (1) placing the dialysis bag in 4 L of distilled water for 12 h, or (2) placing the bag in 1 L of distilled water for 6 h and then in another 1 L of fresh distilled water for another 6 h? EXPLAIN

For each of the following solutions, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

b. For 210.0mL of a buffer solution that is 0.210M in HCHO2 and 0.295M in KCHO2, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

c. For 210.0mL of a buffer solution that is 0.265M in CH3CH2NH2 and 0.240M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.010 mol of NaOH.

For a particle of mass m in a two-dimensional potential well(i.e. particle confined in a 2D box) with sides L1 and L2:
a) Set up the Schrödinger equation for this system.
b) Using separation of variables, derive an expression for thewavefunction
Ψ and for the energy levels of the system. Be sure toshow all of your work for this derivation.
c) For the case of square potential well with side L (i.e.L₁=L₂=L), sketch an energy level diagram forthe nine lowest energy levels, showing degeneracy whereappropriate.

It requires substantial energy to reduce metal ore to pure metal. The reverse process, corrosion, happens spontaneously. The rusting of iron, the tarnishing of silver, and the formation of patina on copper and brass are some common examples of corrosion.

Rusting is the greatest corrosion problem because it occurs rapidly and because so many objects are made of iron and steel. A great deal of the annual production of iron goes simply to replace that lost by rusting. Iron will not rust in dry air or in water that is completely free of air. Oxygen gas and water must be present for iron to rust. Describe chemistry and electrochemistry of corrosion of iron and copper. In each redox reaction, specify the element that is being oxidized, the element that is being reduced, and identify the oxidizing and the reducing agent. Why cars rust more rapidly near the beach or in cold climate where salt is used to de-ice the roads?

Please show all work!

Balance the following reactions in an acidic solution:

Cr2O7^2-(aq)+HNO2(aq)--->Cr^3+(aq)+ NO3-(aq)

Pb^2(aq)+ IO3-(aq)--->PbO2(aq)+I2(aq)