In the following problems answer is given in bracket, I just want the steps how to get them:

(a). Calculate the % of each DRY product when coal is burned stoichiometrically in air. The mass analysis of the coal is: 80% C; 10% H₂; 5% S; and 5% ash.(76.7%N, 22.5%CO₂; 0.8% SO₂)

(b). Find the air fuel ratio for stoichiometric combustion of Butane by volume. Calculate the percentage of carbon dioxide present in the DRY flue gas if 30% excess air is used. (30.95/1; 10.6%)

Make sure you cover both parts as Chegg Question allows at max 4 sub-parts. I want all the steps to get the correct answer.

If 1 grams of sodium bicarbonate are decomposed, determine the combined mass loss (in grams) of water and carbon dioxide that are produced. When a 1.09g mixture of sodium chloride and sodium bicarbonate were heated for several minutes in a crucible and the mass after the first 3 heating intervals remained 0.83 grams.

A 19.3-g mixture of oxygen and argon is found to occupy a volume of 16.2 L when measured at 675.9 mmHg and 43.4^oC. What is the partial pressure of oxygen in this mixture?

Answers:

401 mmHg

338 mmHg

274 mmHg

437 mmHg

239 mmHg

Find the ΔG of the following reaction when there is 1.64 M A in solution. The equilibrium concentrations were found to be 1.00 M A, 0.97 M B, 1.07 M C, 0.55 M D and the temperature is 298K.

2A + B <==> 3C + D

An insultaed container holds 40.30g of water at 23.10 celcius.Sample of copper weighing 7.50g is placed in a dry test tube and heated for 30 min in boiling water at 100.10 celsius. given specific heat of copper is .385 , calculate max temp of water in container after copper metal is added.

Describe 2 methods for modifying the biomaterial surface (do not describe grafted polymer layers).

For each method, briefly describe the following things:

1. How the technique is performed

2. Chemistry examples that can be communicated to the surface

3. 1 example of a healthcare application

In the titration of 25 mL of 0.100 M N2H2 (Kb=8.9x10-7) with .100M HCl, determine the pH at: Please show all steps/ Help please asap

a) the begining of titration

b) after 15 mL of acid has been added

c) after 25 mL of acid has been added

d) after 30 mL of acid has been added

4) In a titration of a 100.0mL 1.00M HA weak acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 49.5 mL of NaOH? K_a = 1.80 x 10^-5 for HA. (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

5) In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 30.9 mL of NaOH? (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

classify the following solution as acids, bases or neutral based on their pH values

water
soda pop
vomit
battery acid
milk
hand soap
coffee
blood
orange juice
drain cleaner
Part B
classify each substance as strong acid, strong base, weak acid, or weak base
H2SO4
HBr
HI
H2SO3
(CH3)2NH
CH3COOH
HCLO4
H3PO4
NAOH
LiOH
can(OH)2
KOH
C6H5COOH
NH3

1) At which point along the titration curve of a weak acid titrated with a strong base does the pH = pK_a

- At the half equivalence volume

- At the equilavence volume

- Before any base is added

- Beyond equilavence volume

2) In a titration of a 100.0mL 1.00M HA weak acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 131 mL of NaOH?   K_a = 1.80 x 10^-5 for HA. (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

3)In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 121 mL of NaOH? (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

4) In a titration of a 100.0mL 1.00M HA weak acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 49.5 mL of NaOH? K_a = 1.80 x 10^-5 for HA. (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

5) In a titration of a 100.0mL 1.00M HCl strong acid solution with 1.00M NaOH, what is the pH of the solution after the addition of 30.9 mL of NaOH? (3 significant figures)

**Remember to calculate the equivalence volume and think about in which region along the titration curve the volume of base falls, region 1, 2, 3, or 4**

Part A) Calculate the solubility (in grams per 1.00×102mL of solution) of magnesium hydroxide in a solution buffered at pH = 12. Part B) Calculate the solubility (in grams per 1.00×102mL of solution) of magnesium hydroxide in pure water.

You are a CEM 262 TA and are preparing a 1.97 M ZnCl2 solution as an unknown for the EDTA titration experiment. The pH must be below what value to avoid precipitation of zinc hydroxide in the solution? The solubility product of Zn(OH)2 is 3×10-16. For this calculation, assume that the solution is ideal.

Six halides: 1-chlorobutane, 2-chlorobutane, Allyl chloride, 2-chloro-2-methylpropane, 1-chloro-2-methylpropane, 2-bromobutane.

SN2: w/ sodium iodide in acetone
SN1: w/ silver nitrate in ethanol

Explain the order of reactivity under SN2 and SN1 conditions by considering alkyl halide structure, nature of the learoup, temperature, solvent, etc.
Please be descriptive and answer them correctly.

Balance the half-reactions assuming that they occur in acidic solution.Express your answer as a balanced half-reaction. Identify all of the phases in your answer.

1) NO3−(aq)→NO(g)

2)Zn(s)→Zn2+(aq)

3)Te(s)→TeO2(s)

4)Sn4+(aq)→Sn2+(aq)