for the calculations performed with the experimental data obtained, which of the following best describes why it is necessary to assume that deltaH and deltaS are temperature independent values. this assumption permits use of a linear equation to fit the data, this assumption allows us to average the data, this assumption allows entropy to be ignored when enthalpy changes are large, this assumption allows entropy to be ignored when enthalpy changes are small, this assumption allows entropy to be ignored when calculating deltaG values

H2S + HNO3 ----> H2SO4 + H2O(l) + NO2 (g)

balance in acidic solution, show all steps.

I found difficulty to differentiate the blank titration and back titration problems/Questions. Can anyone give me the problems/questions of these two titrations..?? (and please give the explanation between these titrations, so i can understand). Thank you so much :)

Calculate percent yield of acetanilidae if you started with 2 mL of aniline and 2 mL of acetic anhydride and obtained only 1.5 grams of acetanilidae. Show detailed work indicating what is the limiting reagent and theoretical tield, etc.

What is the pH of a 2.75 x 10^-3 M solution of potassium fluoride, KF, in water? The K_a for hydrofluoric acid is 3.55 x 10^-5.

please show steps!!

the answer is 7.94

What is the cobalt (II) ion concentration in a solution prepared by mixing 431 mL of 0.444 M cobalt (II) nitrate with 419 mL of 0.276 M sodium hydroxide? The Ksp of cobalt (II) hydroxide is 1.3 × 10-15

1.) A.) CTP stablizes the R or T state? (pick one) of aspartate carbamoyl transferase (ACTase) and acts as a:

a.) positive regulator    b.) negative regulator   c.) a co-factor   d.) competitive inhibitor

B.) regulation of ACTase results in equal numbers of synthesized purines and pyrimidines. explain how this occurs.

C.) What would be the shape of the michaelis-menten curve for this enzyme (like parabolic, sigmoidal,etc)?

Cation Group III Quantitative Analysis Lab?

We just completed our unknown lab, where we are given a test tube with some of the Group III cations (Zn, Cr, Mn, Fe, Al, Ni, Co, and we dont know which are present) and we need to write a discussion about certain chemical concepts, and I am stuck on some.

http://web.cerritos.edu/cshimazu/SitePages/Chem%20112/112%20Experiments/5%20Cation%20III%20Part%20B/Cation%20III%20Part%20B.pdf

(That is the lab handout in case I don't make sense)

So we need to write about equilibrium, and explain it using Le Chatalier's principle and give examples

We can talk about complex ions, like why do some form complex ions and others do not?

Whey do cation III group ions form a hydroxide precipitate in the first place?

Discuss buffers. The buffers we used were NaBiO3, we used it when the solution was acidic , how do they work and why are they important?

Draw line structures corresponding to each name below

1. (3E)-3,7-dimethyl-1,3,6-octatriene

2. 3,6-dimethyl-1,4-cyclohexadiene

Assume you wanted to end up with 38.0 g of copper from the reaction below. What mass of copper (II) sulfate would be required?

Fe + CuSO₄-------> Cu + FeSO₄

Data Table 1. Butane.

A 35.00 mL solution of 0.25M HF is titrated with a standardized 0.1316M solution of NaOH at 25C.

a.What is the PH of the HF solution before titrant is added?

b.How many milliliters of titrant are required to reach the equivalence point?

c.What is the PH at 0.5ml before the equivalence point?

d.What is the PH at the equivalence point?

e.What is the PH at 0.5 ml after the equivalence point?

I got the answer for part A right but I can't seem to get part B or C. Could you please show me working out? Thank you!

Part A

What is the pH of a buffer prepared by adding 0.506mol of the weak acid HA to 0.609mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66

1.What mode of decay is probable for 41/18 Ar ? What mode of decay is probable for ? a.electron capture b. beta emission C.positron emission D.alpha emission

2.

The standard cell potential, E°_cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.

A.−2.57 × 10² kJ, nonspontaneous B. −2.57 × 10² kJ, spontaneous C. −1.28 × 10² kJ, spontaneous D. +2.57 × 10² kJ, nonspontaneous

3. List the given metal ions in order of increasing strength as oxidizing agents, based on the following standard reduction potentials, E°_red .