Calculate the mass of carbon gas produced if 6.000g of K2CO3 reacts with 10.00ml of 2.00M HNO3 identify the limiting reagent as indicated a) if the amount of carbon dioxide collected is part a is 0.3542g, calculate the percent yield for the rection b) if the 0.3542g of carbon dioxide were collected at STP (0C and 1 atm), calculate th volumen of gas collected

Write the formula for the Bronsted-Lowry conjugate acid for each of the following bases.

NH2-

HSO4-

OH-

NH3

H2O

12) You need to reduce the radar cross-section of your company’s new plane.   It already has been built according to principle of radar dispersion, so you must find a materials solution.?

Please explain in clear words. Thanks

8) Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ

Calculate ΔG°rxn for the following reaction.

21 CO2(g) + 28 H2O(g) → 7 C3H8(g) + 35 O2 g)

A) +14518 kJ B) -2074 kJ C) -14518 kJ D) -296 kJ E) +2074 kJ

22) Given the following equation, C3H8(g) + 5 O2(g) → 3 CO2(g) + 4 H2O(g) ΔG°rxn = -2074 kJ

Calculate ΔG°rxn for the following reaction.

7 C3H8(g) + 35 O2(g) → 21 CO2(g) + 28 H2O(g)

A) -14518 kJ B) +2074 kJ C) -2074 kJ D) -296 kJ E) +14518 kJ

29) Given the following equation, H2O(g) + CO(g) → H2(g) + CO2(g) ΔG°rxn = -28.6 kJ

Calculate ΔG°rxn for the following reaction.

5 H2(g) + 5 CO2(g) → 5 H2O(g) + 5 CO(g)

A) +143.0 kJ B) -28.6 kJ C) -143.0 kJ D) +5.72 kJ E) -5.72 kJ

What is the Ka for a weak acid, HA, if a .2 M HA solution has a pH of 4.0?

Will iron(III) hydroxide precipitate from a pH = 1.00 solution with [Fe3+] = 1.0 x 10-5? Ksp Fe(OH)3 = 6.3 x 10-38

A 5.171 g sample of a solid, weak, monoprotic acid is used to make a 100.0 mL solution. 26.00 mL of the resulting acid solution is then titrated with 0.09671 MNaOH. The pH after the addition of15.00 mL of the base is 5.51, and the endpoint is reached after the addition of 47.85 mL of the base.

(c) What is the pK_a of the acid?

What is the potential of a cell made up of Zn|Zn²⁺ and Cu|Cu²⁺ half-cells at 25^o C if [Zn²⁺] = 0.25 M and [Cu²⁺] = 0.15 M?

(Answer should be E = +1.09 V but I need to know how to get to that)

0.560 g He, 20.482 g F₂, and 13.960 g Ar are placed in a 18.4-L container at 25 ^oC. What are the molar concentrations and partial pressures of the gases?
(All values to the nearest 0.0001)

What is the total pressure in the container?

P = atm

which one is more nucleophilic: hydroxide ion (OH) , or ammonia (NH3)? Explain why

A sample mixture of ethyl benzoate (bp 212 C) and dodecane (bp 216.2 C) is injected on two GC columns. Column A has DC710 silicone oil as the stationary phase, and column B uses polyethylene glycol as the stationary phase. Which substance would be certain to elute first from column A and would the same material be expected to elute first from column B? Which column, A or B, would be expected to give the better separation of these two substances?

A particular uncatalyzed reaction proceeds 200 times faster at 45 degrees celcius than at 0 degrees celsius

A. Calculate the activation energy for the reaction

B. when the reaction at 45 degrees celsius is catalyzed, the reaction rate increases by a factor or 500. calculate the activation energy for the catalyzed reaction?

A gaseous sample of a certain compound follows the postulates of the kinetic molecular theory and has a most probable speed pf 264.13 m/s at a certain temperature.

A) The molecules in this sample are a binary compound of sulfur and nitrogen that is 30.4 mass percent nitrogen. The molar mass of this compound is between one hundred fifty and two hundred g/mole. Determine the molecular formula of this compound and the temperature of this sample in degrees Celsius.

B) This gaseous sample, at the above temperature, is in a 5.00 L container at a pressure of 280 torr. Determine the collision frequency of these molecules with a 2.00 mm² area of the container wall. Express your answer in moles/second.

Carbonyl fluoride, COF2, is an important intermediate used in the production of fluorine-containing compounds. For instance, it is used to make the refrigerant carbon tetrafluoride, CF4 via the reaction

2COF2(g)⇌CO2(g)+CF4(g),    Kc=7.40

If only COF2 is present initially at a concentration of 2.00 M, what concentration of COF2 remains at equilibrium?

Where I get stuck is figuring out how to multiply (x)(x)/ (2.00-2x)^2 I know this is easy math but can you please work it out step for step so that I can see exactly how you go the answer.