A fire extinguisher has a pressure of 12 atm at 25∘C.What is the final pressure, in atmospheres, when the fire extinguisher is used at a temperature of 63 ∘C, if Vand n are constant?

P=

What are the rules for net ionic equations? I know you must follow the solubility chart, but I'm confused about the other aspects. When the compound is solid, gas or liquid, I don't break apart the compound right? Unless the compound is a strong acid and base? I already know the steps of finding the net ionic equation. I'm just not sure about the rules. So if you could provide an example for the different reactions, can you also include the differences when using the rules?

In the williamson ether synthesis of n-butyl methyl ether from 1-bromobutane, sodium, and ethanol, how could the purity as well as the percent yield of the product be improved?

Consider the following reaction:

CO(g)+2H2(g)⇌CH3OH(g)CO(g)+2H2(g)⇌CH3OH(g)

The reaction between COCO and H2H2 is carried out at a specific temperature with initial concentrations of COCO = 0.32  M M and H2H2 = 0.52  M M. At equilibrium, the concentration of CH3OHCH3OH is 0.15  M M.

Find the equilibrium constant at this temperature.

Express your answer using two significant figures.

Please answer and exaplain ALL 4 parts! Thank you!

A 3.00 mL aliquot of 0.001 M NaSCN is diluted to 25.0 mL with 0.2 M Fe(NO3)3 and 0.1 M HNO3.

1. How many moles of SCN- are present?

2. If all of the SCN- is complexed with Fe3+ to form FeNCS2+, what is the molar concentration of FeNCS2+?

3. For preparing a set of standard solutions of FeNCS2+, the equilibrium molar concentration of FeNCS2+ is assumed to equal the initial molar concentration of the SCN- in the reaction mixture. Why is this assumption valid?

4. The blank solution used to calibrate a spectrophotometer is 10.0 mL of 0.2 M Fe(NO3)3 diluted to 25.0 mL with 0.1 M HNO3. Why is this solution preferred to simply using de-ionized water for the calibration?

What is the concentration of a solution created by mixing 25g of C₃H₆O_(L) (D = 0.774 g/mL) with 25g of CH₄O_(L) (D = 0.890 g/mL)?

Which of the following has the highest boiling point? Please provide an explanation on how to solve this!

a. CH₃OH                b. CH₃Cl                  c. CH₃SH                 d. CH₃CH₃                       e. CH₃F

HClO is a weak acid (Ka=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.037 M in NaClO at 25 °C?

A 27.7 mL sample of 0.314 M ethylamine, C2H5NH2, is titrated with 0.325 M nitric acid. The pH before the addition of any nitric acid is .

Use the Tables link in the References for any equilibrium constants that are required.

1. What is the molarity of a solution that contains 18.7 g of KCl (MW=74.5) in 500 mL of water?
   
2. 25 g of NaOH (MW = 40) is added to 0.5 L of water. What is the molarity of this solution if an additional 0.25 L of water is added to this solution?
   
3. How many grams of H₂SO₄ (MW = 98) are in 750 mL of 3 N H₂SO₄?
   
4. What is the normality of a solution that contains 280 g of NaOH (MW=40) in 2000 mL of solution?
   
5. A serum potassium is 19.5 mg/100 mL. This value is equal to how many mEq/L (MW = 39)?

You are given a series of 5 tubes, each of which contains 5 mL of saline. To the first tube is added 1 mL of serum, and a serial dilution using 1 mL is carried out in the remaining tubes.

6. What is the dilution in the first tube?
7. What is the final dilution in the third tube
8. The third tube was run, and the triglyceride concentration was 3 mg/dL. Give the triglyceride concentration in the 1^st tube:
9. What is the concentration of the original specimen?
10. What result do you report out?

Consider an ionic compound, MX2MX2 , composed of generic metal MM and generic, gaseous halogen XX .

• The enthalpy of formation of MX2MX2 is ΔH∘f= −817ΔHf∘

• The enthalpy of sublimation of MM is ΔHsub= 115ΔHsub

• The first and second ionization energies of MM are IE1= 717IE1 and IE2= 1395

• The electron affinity of XX is ΔHEA= −323 kJ/mol. (Refer to the hint).

• The bond energy of X2X2 is BE= 165 kJ/mol.

Determine the lattice energy of MX2MX2 .

ΔHlattice=______kJ/mol

I start with 3 mL of [Ru(bpy)3](PF6)2 solution. Every time Add 100 uL volume of DPA solution with 0.05M. Do it five times, the total amount of DPA is 500ul

500ul

I am so confused about how to calculate the concentration of DPA in each adding