Rank the following in order of increasing polarity: CH2Cl2, CF2Cl2, CH2Br2, CBr4

A diver breathes a helium and oxygen mixture with an oxygen mole fraction of 0.052. What must the total pressure be for the partial pressure of oxygen to be 0.22 atm ?

A solution was prepared by weighing out 6.20 grams of sodium benzoate, NaC7H5O2 along with 2.25 grams of benzoic acid, HC7H5O2, and was dissolved in 750.0 mL of water. What is the pH of this solution given that the Ka for benzoic acid is 6.61 X 10-5 .

The pKb values for the dibasic base B are:
pKb1= 2.10
pKb2= 7.70
Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.75 M B(aq) with a 0.75 M HCl(aq).
a. before addition of any HCl
b. after addition of 25.0 mL of HCl
c. after addition of 50.0 mL of HCl
d. after addition of 75.0 mL of HCl
e. after addition of 100.0 mL of HCl

please show your work as I really do want to understand the process. thank you so much :)

A.) An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 35.0 atm and releases 73.8 kJ of heat. Before the reaction, the volume of the system was 7.00 L . After the reaction, the volume of the system was 3.00 L . Calculate the total internal energy change, ΔE, in kilojoules.

B.) It takes 45.0 J to raise the temperature of an 10.6 g piece of unknown metal from 13.0∘C to 24.1 ∘C. What is the specific heat for the metal?

C.)The molar heat capacity of silver is 25.35 J/mol⋅∘C. How much energy would it take to raise the temperature of 10.6 g of silver by 11.6 ∘C?

D.)What is the specific heat of silver?

1.) Explain why the first derivative of the titration curve can be used to identify the equivalence point of an acid-base titration (or equivalence points for polyprotic acids).

2.)  Explain the effect of pKa on endpoint detection for the titration of a weak acid with a strong base:

3.) Explain the effect of acid strength (molarity) on endpoint detecton for the titration of a weak acid with a strong base.

In gluconeogenesis, what are it's thermodynamics and enzymatic regulations?

write and label the half-reactions for the reduction of I₃^- (aq) by S₂O₃^2- (aq)

two procedures:

1. a microscale cis-trans isomerization of an alkene

2. a miscroscale addition of bromine to fumaric acid

For each procedure:

a. predict which alkene will predominate at equilibrium (please explain)

b. predict the stereochemistry of the products formed if the addition of bromine to fumaric acid occurs via: syn addition, anti addition, and stereorandom addition

Thank You

experment (Nylon-6,6)
1- 5-7 sentences for result .
2- 5-7 sentences for the conclusion

what is the purpose of the trap that is used during a vacuum distillation performed with an aspirator?

1) If the pI for a particular amino acid is 7.5, at which pH will the net charge on the molecule be zero?

2) Calculate the pH of 0.00756 M HNO₃.

3) The isoelectric point of an amino acid is defined as:

a. the pH at which it exists in the basic form

b. the pH equals the pKa

c. the pH at which it exists in the acidic form

d. the pH at which the amino acid exits in the zwitterion form

4) Given the following reaction, the equilibrium expression will be:
4 CuO (s) + CH₄ (g) ↔ CO₂ (g) + 4 Cu (s) + 2 H₂O (g)

a. [Cu]⁴/[CuO]⁴

b. [CuO]⁴/[Cu]⁴

c. [CO₂][H₂O]²/[CH₄]

d. [CuO]/[Cu]

The following reaction is exothermic. Which of the following will drive the reaction to the right (towards products)?
CH₄ (g) + 2 O₂ (g) ↔ CO₂ (g) + 2 H₂O (g)

a. An increase in temperature

b. A decrease in temperature

c. The addition of CO₂

d. The removal of CH₄

Hydrogen gas, H2, reacts with nitrogen gas, N2, to form ammonia gas, NH3, according to the equation

3H2(g)+N2(g)→2NH3(g)

a. How many grams of H2 are needed to produce 11.70 g of NH3?

b. How many molecules (not moles) of NH3 are produced from 4.42×10⁻⁴ g of H2?

63. Ethylene, C2H4, used to make polyethylene plastics, can be made from ethane, C2H6, one of the components of natural gas. The heat of reaction for the decomposition of ethane gas into ethylene gas and hydrogen gas is 136.94 kJ per mole of C2H4 formed, so it is endothermic. The reaction is run at high temperature, in part because at 800-900 °C, the equilibrium constant for the reaction is much higher, indicating that a higher percentage of products forms at this temperature. Explain why increased temperature drives this reversible chemical reaction in the endergonic direction and why this leads to an increase in the equilibrium constant for the reaction. C2H6(g) = C2H4(g) + H2(g)

The following equation represents the decomposition of a generic diatomic element in its standard state.

1/2 X₂ (g) = X (g)

Assume that the standard molar Gibbs energy of formation of X(g) is 5.40 kJ·mol–1 at 2000. K and –53.08 kJ·mol–1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.

K at 2000. K = ?

K at 3000. K = ?

Assuming that ΔH°rxn is independent of temperature, determine the value of ΔH°rxn from these data.

ΔH°rxn = ? kj x mol^-1