Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is

S2(g) + C(s) <---> CS2(g)

How many grams of CS2(g) can be prepared by heating 21.0 moles of S2(g) with excess carbon in a 9.15 L reaction vessel held at 900 K until equilibrium is attained?

Determine the catalyst activity of trypsin.

Develop a procedure to determine the ideal gas law constant R from:

NaHCO3 (s) + CH3COOH (aq)--> NaCH3COO (aq) + CO2(g) + H20 (l)

so that different amounts of CO2 will be produced and collected from NaHCO3 powder and ~0.5 mol/L CH3COOH solution and the following equipment: test tubes, small vials, stopper, tubing, water trough, graduated cylinders, and erlemeyer flasks. Please help!

Use the thermodynamic arguement to explain why the perfectly folded protein is only marginally stable compared to its unfolded form.

Use the same equation to explain why higher temperatures denature proteins.

Which of the weak forces is the most important in the overall protein stability?

How does the packing found inside a fractional column work to separate a mixture of two components?

Using your average K_eq value (.3948), please calculate what the equilibrium concentrations of Fe³⁺ , SCN^- , and FeSCN²⁺ in a solution made by combining 10.00mL of 0.0020M Fe(NO₃)₃ and 10.00mL of 0.0020M KSCN.

Explain the effects of each of the following on the rates of gluconeogenesis and/or glycolysis.

A. Increasing the concentration of blood glucose.

B. Increasing the concentration of glucose-6-phosphate.

C. Increasing the concentration of fructose-1,6-bisphosphate.

D. Increasing the levels of ATP.

E. Increasing the concentration of AMP.

F. Decreasing the concentration of fructose-2,6-bisphosphate

G. Increasing the concentration of acetyl CoA

H. Increasing the concentration of citrate.

3/ At 2000 K , nitrogen gas and oxygen gas combine to form nitric oxide according to the following reaction: N2(g) + O2(g) ⇌ 2NO(g) ΔH = +1.81 KJ

with an equilibrium constant K of 4.1 x 10^-4. If 0.50 mole of N2 and 0.86 mole of O2 are put into a 2.0 L container at 2000 K , what would the equilibrium concentrations of all species be ?

4/ For the reaction in question #3. How would the following changes effect the equilibrium ? Each change occurs independently of the others. Increase temperature. Decrease pressure. Decrease [O2(g)]. Increase [NO(g)]

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.140 M HClO(aq) with 0.140 M KOH(aq). The ionization constant for HClO is 4.0x10^-8. (a) before addition of any KOH (b) after addition of 25.0 mL of KOH (c) after addition of 35.0 mL of KOH (d) after addition of 50.0 mL of KOH (e) after addition of 60.0 mL of KOH

Part A

A volume of 105 mL of H2O is initially at room temperature (22.00 ∘C). A chilled steel rod at 2.00 ∘C is placed in the water. If the final temperature of the system is 21.00 ∘C , what is the mass of the steel bar?

Use the following values:

specific heat of water = 4.18 J/(g⋅∘C)

specific heat of steel = 0.452 J/(g⋅∘C)

Part B

The specific heat of water is 4.18 J/(g⋅∘C). Calculate the molar heat capacity of water?

What is the molarity of a solution of s2o32- if 58 ml were required to titrate 42 ml of a 0.2M solution of IO3-

A) Does the pH increase, decrease or remain the same on the addition of the of the following?

B) Which of the following (select all that apply) gives a buffer solution when equal volumes of the two solutions are mixed?

Fluoride Selective Ion Electrode. Describe how a fluoride selective ion electrode measures the fluoride ion concentration and explain why the potential approaches 0 at high concentrations

7. Given the standard reduction potential for the following two half-cell reactions (in the presence of 1.00 M HCl):

Fe3+ + e <==> Fe2+, E0 = + 0.68 V

AsO4 - + 2H+ + 2e <==> AsO3 - + H2O, Eo = +0.559 V.

Please calculate the system potential at the equivalence point when Fe3+ was used to titrate AsO3 - in the presence of 1.00 M HCl.

Answer: 0.60 V