When 1.90 mol CO2 and 1.90 mol H2 are placed in a 3.00-L container at 395 ∘C, the following reaction occurs: CO2(g)+H2(g)⇌CO(g)+H2O(g).?

Part A
If Kc = 0.802, what are the concentrations of CO2 in the equilibrium mixture?
Part B
If Kc = 0.802, what are the concentrations of H2 in the equilibrium mixture?
Part C
If Kc = 0.802, what are the concentrations of CO in the equilibrium mixture?
Part D
If Kc = 0.802, what are the concentrations of H2O in the equilibrium mixture?

During a titration, a student used 31.92 ml of a .1000 M NaOH (aq) to neutralize 30.0 ml of a . 2488 M oxalic acid solution.

1. Consider the following reaction:

3CH4(g)→C3H8(g)+2H2(g)

Calculate ΔG at 298 K if the reaction mixture consists of 41 atm of CH4, 0.011 atm of C3H8, and 2.1×10⁻² atm of H2.

Express the Gibbs free energy in kilojoules to two significant digits.

2. The element gallium (Ga) freezes at 29.8 ∘C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol.

Calculate the value of ΔS when 61.0 g of Ga(l) solidifies at 29.8 ∘C. in J/K

What is the molar solubility of Fe(OH)₃ in a solution buffered at pH = 4.52? (See the appendix.)
M

What is the molar solubility at pH = 8.16?
M

A sample of ammonia gas is completely decomposed to nitrogen andhydrogen gases over heated iron wool. If the total pressure is 639mmHg, calculate the partial pressure of N2 and H2. Enter your answers in scientific notations

Consider 25 ± 1 (n=5) and 26 ± 1 (n=6); The uncertainty listed is the standard deviation. Are these two measurements significantly different at the 95% confidence limit ?  

If 4.90 g of CuNO3 is dissolved in water to make a 0.850 M solution, what is the volume of the solution?

Identify the following statements as true or false. (Use the drop-down menu and select "True" or "False" for each. You must get all 6 correct.)
1. The entropy of the universe is constant; the energy of the universe decreases towards a minimum.
2. If a reaction is spontaneous, the reverse reaction is non-spontaneous.
3. If a process decreases the randomness of the particles of a system, the entropy of the system decreases.
4. Both ΔS_sys and ΔS_surr must equal zero at equilibrium.
5. All systems become more disordered spontaneously.
6. The boiling of water at 105°C and 1 atm is a spontaneous process.

12. 175 g of Fe at 15.0oC is mixed with 225 g of H2O at 95.0oC. What is the final temperature of the mixture? The specific heats of iron= 0.448 J/g oC and water = 4.184 J/g oC). (keep in mind the following: heat gained + heat lost = 0 and q=mass x heat capacity x T)

I need yo know this answer by midnight tonight. thanks.

you will need to construct your own data sheet for this experiment.

DATA ANALYSIS steps 1-2:
The colorimeter wsa used to measure teh absorbance of each of a series of [FeSal]+ solutions. A standard curve was constructed by plotting the absorbance vs. the concentration (M). The slope and y-intercept were found to be 1510 M^-1 and 0.001, respectively.
PROCEDURE:
An aspirin sample was prepared, following the procedure given in the experiment: hydrolyzing the 0.139 g of it with 5 mL of a 1 M NaOH (reaction 1), diluting this mixture to 50.0 mL (forming solution A), and taking a 1.00 mL aliquot of this solution an diluting it to 50.00 mL with 0.02 M Fe(III) (forming solution B - reaction 2). The absorbance of solution B was measured to be 0.366.
DATA ANALYSIS step 3:
(a) Use the measured absorbance and the standard curve's slope and y-intercept to calculate the concentration of [FeSal]+ in solution B.

(b) How many moles of [FeSal]+ were in the 50.00 mL of solution B?

(c) How many moles of sodium salicylate were in the 1.00 mL aliquot of solution A used to prepare soution B?
Hint: look at the stoichimetry of reaction (2) in the experiment to see how the moles of sodium salicylate realte to the moles of [FeSal]+.

(d) Given the number of moles of sodium salicylate in 1.00 mL of solution A (calculated above), how many moles are in the 50.00 mL of solution A?
Hint: This is not a dilution or Beer's Law problem. It is a simple multipication.

(e) Based upon the number of moles of sodium salicylate calculated in part (d), how many moles of acetlsalicylic, C9H8O4, were in the aspirin sample?
Hint: look at the stoichiometr of reaction (1) in the expt.

(f) Use the mass of the aspirin sample (given in the PROCEDURE section above) and the answer to part (e), coverted to grams to calculate the mass percent of acetlsalicyclic acid, C9H8O4, in the aspin sample.

2. A one liter of solution phosphate buffer is made so that it is 1.00M in NaH2PO4 and 1.50M in Na2HPO4. If the pka of NaH2PO4 is 7.21 assuming the volume negligible change upon addition of acid or base calculate?

a. the Ph of buffer?

b. the resulting pH after addition of 0.25 mol of NaOH?

c. the amount of NaOH that would have to original buffer to bring pH upto 8.0

1) During the work-up procedure of our second reaction (“Hydrogenation of a Chalcone”), the following steps are performed:

a) Add 15 mL of brine and 10 mL of ethyl acetate to the mixture. Shake vigorously, then separate the ethyl acetate layer from the aqueous phase. Store the ethyl acetate layer in a dry, clean Erlenmeyer flask.

b) Extract the aqueous phase again with an additional 5 mL of ethyl acetate.

c) Combine the two ethyl acetate solutions and wash this ethyl acetate layer with 5

mL of brine. Drain the aqueous phase and pour the ethyl acetate solution into a

clean 25-mL Erlenmeyer flask.

d) Dry the organic phase with anhydrous magnesium sulfate for 5 min.”

Why are we performing each of the four steps mentioned above? (What is the purpose?) Please explain.