The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reactions of a number of such steps for methane gas is
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 145 mL of methane at STP, 885 mL of oxygen at STP, and 59.5 mL of NO at STP in a 1.8 −L flask. The reaction is allowed to stand for several weeks at 275 K .

If the reaction reaches 92.0% of completion (92.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K ?

If the reaction reaches 92.0% of completion (92.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K ?

What is the total pressure in the flask?

Using the set of smallest whole number coefficients to balance the redox equation

MnO₄^- + NO₂^- ---> MnO₂ + NO₃^-

in basic solution, you get

a) 2 OH^- on the right.

b) 3 OH^- on the left.

c) 1 H₂O on the right

d) 3 H₂O on the left

TLC analysis of an unknown sample using pure ethyl acetate as a developing solvent gives a single spot with an Rf value of 0.08.

A. Explain why this result doesn't guarantee that the sample is a pure compound.

B. Suggest two changes that could be made to the experiment to improve the analysis of the unkonwn sample.

(1)   What do you assume the entropy S for a perfect crystal when T = 0?

(2)   Is the S(0) still zero if the crystal is not perfect? Why?

(3)   How to calculate dS when under the constant pressure and c_p is given?

(4)   How to calculate the entropy of H₂O at 500 K?

(5)   How to calculate the entropy change for a chemical reaction if you can find the S for each chemical?

(6)   For an isolated thermodynamic system, dS ³ 0. That is, dS = 0 for a reversible process and dS > 0 for an irreversible process (spontaneous process).

A flask contains 30.5 g of oxygen gas, 45.7 g of sulfur dioxide gas and 23.9 g of fluorine gas. If the total pressure of the flask is 1.45 atm, what is the partial pressure of sulfur dioxide gas in the flask?

Integrated Rate Laws: Working with Zero Order Reactions Experiments have shown the following reaction to be zero order with a rate constant = 2.50 10-1 M/sec. A → B + 2 C If you started with [A] = 2.600 M, how many minutes until the concentration of A = 2.300 M? .02 Correct: Your answer is correct. minutes How many minutes until the concentration of C reaches equals 0.899999999999999 M? 1.73 Incorrect: Your answer is incorrect. minutes

A solution is prepared by mixing 25.0g pentane with 75.0g hexane. The density of the solution is 0.65g/mL. Determine the molarity and the molality of the solution.

*Please be as thorough as possible without skipping any steps. Thank you!

A voltaic cell has one half-cell with a Cu bar in a 1.00 M Cu2+ salt and the other half-cell with a Cd bar in the same volume of a 1.00 M Cd2+ salt.

(a) Find E o cell , ΔG o , and K. Report your answers to the correct number of significant figures.

E o cell = V

ΔG o = × 10 J

K = × 10

(b) As the cell operates, [Cd2+] increases; find E cell when [Cd2+] is 1.95 M.

E cell = V

(c) Find E cell , ΔG, and [Cu2+] at equilibrium.

E cell = V

ΔG = J

[Cu2+] = × 10 M

Using the sample in question 3, how many counts per second would be observed when the detector is 10 meters away from the sample? 5. If a 10 gram sample of a radioactive substance has a half-life of 6000 years, how much would be present after 8000 years? 6. If Nitrogen-14 absorbs an alpha particle and then emits a Hydrogen-1, what is the resulting nucleus? 7. If Au-185 emits an alpha particle, what is the nucleus formed? 8. What nucleus emits an alpha particle and forms Th-234? 9. If Th-234 emits a beta particle, what nucleus is formed? 10. If Nitrogen-14 absorbs a neutron and then emits a Hydrogen-1, what nucleus is formed

Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T.

ΔH∘rxn=− 132 kJ ; ΔS∘rxn= 260 J/K ; T= 310 K

ΔH∘rxn= 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 310 K

ΔH∘rxn=− 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 310 K

ΔH∘rxn=− 132 kJ ; ΔS∘rxn=− 260 J/K ; T= 563 K

A. Calculate KP at 298 K for the reaction NO(g)+12O2(g)→NO2(g) assuming that ΔH∘R is constant over the interval 298-600 K.

B. Calculate KP at 486 K for this reaction assuming that ΔH∘R is constant over the interval 298-600 K.

Thank you

1. How many grams of ethylene glycol, C2H4(OH)2, are needed per kilogram of water to protect radiator fluid against freezing down to -10°C?

2. For benzene, C6H6, the freezing point constant, Kf, is 5.12 K oC/m and its normal freezing point is 5.5°C. What is the freezing point of a solution containing 100.0 g of benzene and 20.0 g of naphthalene (C10H8)?

3. When 5.0 g of an unknown substance is dissolved in 100.0 g of water, the freezing point of the solution decreases by 1.5°C. What is the molar mass of the unknown substance if the compound does not dissociate to form ions in solution?

4. If 2.00 moles of a substance is dissolved in 1.00 kg of water, the freezing point of the solution decreases by 7.44°C. Does this substance dissociate to form ions in solution? Explain why.

5. Calculate the freezing point of a 0.2 m CaCl2 aqueous solution, assuming it dissociates completely to form ions in solution.

At 25ºC the osmotic pressure of an aqueous CaCl2 solution is 9545.4 torr; the solution has a density of 1.71 g/mL. Calculate the new boiling point of this solution in Celsius. Assume the normal boiling point of water is 100ºC. (MMCaCl2 = 110.984 g/mol; Kb, H2O = 0.512 ºC/m; Kf, H2O = 1.86ºC/m)

I've literally asked this question 4 times now... its pretty sad people can't read as smart as they are to be able to answer these questions....

What amount of energy is required to change a spherical drop of water with a diameter of 1.60 mm to SIX (6) smaller spherical drops of equal size? The surface tension, γ, of water at room temperature is 72.0 mJ/m2. PLEASE DO NOT GIVE ME ANSWER FOR FIVE (5) ITS SIX (6)!