For the reaction 2 A(aq) <---> B(aq) + C(aq), the standard Gibbs free enthalpy change is 1.69 kJ at 25oC. The initial concentration of A(aq) is 0.549 M, the initial concentration of B(aq) is 0.327 M, and the initial concentration of C(aq) is 0.234 M. What would be the concentration of A(aq) (in mol/L) once we attain equilibrium (we are still at 25oC)?

If 20.00 mol of helium gas is at 17.0 ∘C and a gauge pressure of 0.320 atm .

Calculate the temperature in celcius if the gas is compressed to precisely half the volume at a gauge pressure of 1.00 atm. Original volume is 0.3608m3

Calculate the height of a column of carbon tetrachloride, CCl4(l), with a density of 1.59 g/mL that exerts the same pressure as a 15.2 cm column of Mercury, Hg(l), that has a density of 13.6 g/ml. Express your answer in meters. Please only enter the numerical value of your answer.

A sample of a concentrated fluorescent reagent was serially diluted with three steps using a variable volume 100 to 500 μL micropipetor and 10.00 mL Class A volumetric flasks. The concentrated reagent had a fluorescent signal of 653.4 and the diluted sample produced 0.057 fluorescence units. Unfortunately the steps followed for the dilution were lost. What were those steps?

In your own words, clearly explain the process of electrolysis of water. Include a description of the equipment involved, as well as the resulting chemical reaction(s).

3. The

Part A What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. (Express answer to 3 decimal places) Part C What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.

A voltaic cell is constructed that uses the following reaction and operates at 298 K:
Zn(s)+Ni2+(aq)→Zn2+(aq)+Ni(s).

a. What is the emf of this cell when [Ni2+]= 2.10 M and [Zn2+]= 0.160 M ?

b. What is the emf of the cell when [Ni2+]= 0.100 M and [Zn2+]= 0.860 M ?

Thanks!

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 as follows:
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, 895 mL of oxygen at STP, and 54.5 mL of NO at STP in a 2.0 −Lflask. The reaction is allowed to stand for several weeks at 275 K.

Part A

If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K?

Enter your answers numerically separated by commas.

Part B

If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K?

Enter your answers numerically separated by commas.

Part C

What is the total pressure in the flask?

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute.

a)Calculate the freezing point of a solution containing 10.8

g FeCl3 in 172 g water.

b)Calculate the boiling point of a solution above.

c)Calculate the freezing point of a solution containing 4.3 % KCl

by mass (in water).

d)Calculate the boiling point of a solution above.

e)Calculate the freezing point of a solution containing 0.155 m MgF2.

f)Calculate the boiling point of a solution above.

Which of the following are true statements about equilibrium systems?

True/False For the following reaction at equilibrium:
                       2 H₂(g) + O₂(g) ⇌ 2 H₂O(g)
                       the equilibrium will shift to the left if the volume is doubled.

True/False For the following reaction at equilibrium:
                       H₂(g) + F₂(g) ⇌ 2HF(g)
                       removing H₂ will decrease the amount of F₂ present once equilibrium is reestablished.

True/False For the following reaction at equilibrium:
                       CaCO₃(s) ⇌ CaO(s) + CO₂(g)
                       adding more CaCO₃ will shift the equilibrium to the right.

True/False Increasing the temperature of an exothermic reaction shifts the equilibrium position to the right.

True/False For the following reaction at equilibrium:
                       CaCO₃(s)⇌ CaO(s) + CO₂(g)
                       increasing the total pressure by adding Ar(g) will shift the equilibrium to the right.

A piece of copper wire is 50ft long and has a dimater of 2.0 mm. Copper has a denisty of 8.92 g/cm³. What is the mass of copper? Express the answer in kg. (1ft = 30.48 cm, 1 cm = 10 mm and Volume is 3.14 x r²x1)

Please explain and help ! :(

One electrode compartment consists of an aluminum strip placed in a solution of Al(NO3)3, and the other has a nickel strip placed in a solution of NiSO4. The overall cell reaction is

2Al(s)+3Ni2+(aq)?2Al3+(aq)+3Ni(s)

1. What is being reduced?

2. Write the half-reactions that occur in the two electrode compartments.

anode reaction:

cathode reaction:

How many grams of Na2CO3 should be mixed with 5.00 g of NaHCO3 to produce 100 mL of buffer with a pH of 10.00? What volume of 0.01 M NaOH must be added to this solution to achieve a pH of 11.25? (pKa1 is 6.35; pKa2 is 10.53)

Using energy level diagrams, predict the relative stability of a Br₂ molecule as well as the first excited state.