A pure, low molecular weight hydrocarbon gas is burnt in a furnace giving a flue gas containing

10.8% CO 2 , 3.8% O 2 and the remainder nitrogen. Calculate the atomic ratio, H/C, and from this

the formula of the fuel. Note that this analysis is on a dry basis.

2nd part:

Calculate the analysis of the flue gases resulting from the combustion of ethane with 100%

excess air. Give the results on a dry basis.

A mixture of oxygen and nitrogen gases is maintained in a 7.17 L flask at a pressure of 1.53 atm and a temperature of 41°C. If the gas mixture contains 8.88 grams of oxygen, the number of grams of nitrogen in the mixture is  g.

A mixture of methane and argon gases, in a 6.68 L flask at 43 °C, contains 1.35 grams of methane and 5.20 grams of argon. The partial pressure of argon in the flask is  atm and the total pressure in the flask is  atm.

At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.200 M[N2]=[O2]=0.200 M and [NO]=0.400 M.[NO]=0.400 M.

N2(g)+O2(g)−⇀↽−2NO(g)N2(g)+O2(g)↽−−⇀2NO(g)

If more NONO is added, bringing its concentration to 0.700 M,0.700 M, what will the final concentration of NONO be after equilibrium is re‑established?

[NO]final=

Gaseous ethane CH3CH3 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. If 2.19g of carbon dioxide is produced from the reaction of 2.7g of ethane and 3.2g of oxygen gas, calculate the percent yield of carbon dioxide. Round your answer to 2 significant figures.

What is the relationship between % transmittance and concentration?

explain how a QIAprep spin miniprep purification column (( with silica gel functional group (silanol))) works in regards to pH / pKa for binding and elution of DNA

How much heat is evolved in converting 1.00 mol of steam at 150.0 ∘C to ice at -50.0 ∘C? The heat capacity of steam is 2.01 J/(g⋅∘C) and of ice is 2.09 J/(g⋅∘C).

Describe an ether synthesis.

A) what is the definition of an "amhiprotic" substance?

B) Illustrate with two equations how the dihydrogen phosphate anion is amphiprotic:

C) Validate/illustrate your answer to part (B) with two balanced equations and their Keqs.

D)Would a solution of potassium dihydrogen phophate be acidic or basic?

Answer the following chemistry question:

3. (a)  The pKa for ferric ion Fe(+3) is 2.   The pKa for cupric ion Cu(+2) is 9.  

              Which is a stronger Bronsted acid?  Give and explain two reasons for the ten million-fold difference in their acidities

b)  The K_sp for silver tarnish, that is the black Ag₂S, is 10^-39, one of the smallest values indicating a VERY insoluble solid.  Why is silver sulfide so insoluble?

Compare the energy cost, in ATP equivalents, of synthesizing

stearate from mitochondrial acetyl-CoA to the energy recovered by

degrading stearate to CO2

.

Iron-56 has one of the highest binding energies of all nuclides. Calculate its nuclear binding energy in
kJ per mol nucleon. 1 amu is equivalent to 1.492 ´ 10^-10 J.

Ethanol melts at -114.0 ∘C. The enthalpy of fusion is 5.02 kJ/mol and the enthalpy of vaporization is 38.6 kJ/mol. The specific heats of solid and liquid ethanol are 0.970 J/g⋅K and 2.30 J/g⋅K, respectively.

How much heat is needed to convert 39.0 g of solid ethanol at -160.0 ∘C to liquid ethanol at -35.0 ∘C ?

I am really confused on this, any help would be greatly appreciated. Thanks!

Add the physical state for each substance in the following aqueous reactions. Then write and balance a net ionic equation for each reaction. (a) Cr2(SO4)3 + KOH → Cr(OH)3 + K2SO4 (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) AP 17 (b) K2CrO4 + PbCl2 → KCl + PbCrO4 (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) AP 34 (c) Na2SO3 + H2SO4 → Na2SO4 + H2O + SO2 (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) (aq) (s) (g) (l) AP 55

A one molar solution of the weak base methylamine, CH₃NH₂ is diluted with water until the concentration is ½ molar. Which of the following statements are correct for this process?

1. [OH^-] / [CH₃NH₃⁺] remains constant.

2. pH decreases.

3. The % ionization decreases.

• A.

  1 only

• B.

  3 only

• C.

  1 & 2 only

• D.

  2 only

• E.

  2 & 3 only