Gastric juice (pH 1.5) is produced by pumping HClfrom blood plasma (pH 7.4) into the stomach. Calculate the amount of free energy required to move H+ at 37 °C under cellular conditions? How many moles of ATP must be hydrolyzed to provide this amount of free energy? How many molecules of ATP is that? he free energy change for ATP hydrolysis under cellular conditions is about -58 KJ/mol.

**Ignore the effects of the transmembrane electrical potential**

Find a specific example of where nuclear power/energy/technology is being used and write and telling us about your example. Make sure to include the specific element information. State the Isotope name. When was it discovered? What is the half-life? What is the chemical reaction? How does it decay? (for example, "it decays with the emission of an alpha-particle") Include what nuclear processes are being used and how it might be a benefit to man-kind or a danger. Also include information about any controversies that may surround your example, along with your own opinion about it.

You can smell the odor of cooking onions from far away. You can smell the odor of cooking onions from far away. As onions are heated the volume of the gas causing the smell increases. The pressure of the gas which causes the smell is very high. The random movement with high velocities leads to diffusion of the gas particles. Since gas particles are very small, they can penetrate through large volumes of air.

Here are the answers for the previous part of this question, it has multiple parts (these are all at 25 degrees):
A) 2CH4(g)→C2H6(g)+H2(g)
ΔH∘rxn 64.6 kJ
B) 2NH3(g)→N2H4(g)+H2(g)
ΔH∘rxn 187.2 kJ
C) N2(g)+O2(g)→2NO(g)
ΔH∘rxn 182.6 kJ
D) 2KClO3(s)→2KCl(s)+3O2(g)
ΔH∘rxn -77.6 kJ
E) For the reaction in part A calculate ΔS∘rxn at 25 ∘C.
ΔS∘rxn -12.7

I NEED:
F) For the reaction in part B calculate ΔS∘rxn at 25 ∘C.
G) For the reaction in part C calculate ΔS∘rxn at 25 ∘C.
H) For the reaction in part D calculate ΔS∘rxn at 25 ∘C.

Calculate the pH of 0.1 mol/L H2SO4 ; you are given the second dissociation constant of the acid to be 0.01.

Use the table of thermodynamic data in your text, a Chemistry/Physics CRC, or the internet (but be careful with data off the internet), to calculate the molar enthalpy of the following reactions:

1) An aqueous solution of sodium hydroxide reacts with an equeous solution of hydrochloric acid, yielding water.

2) An aqueous solution of sodium hydroxide reacts with an aqueous solution of ammonium chloride, yielding aqueous ammonia, NH₃, and water.

3) An aqueous solution of hydrochloric acid reacts with aqueous ammonia, NH₃, yielding aqueous ammonium chloride.

The reaction A(aq) ---> B(aq) + C(aq) is a first order reaction. The half-life of A(aq) is 86.6 s at 25.0^oC and its half-life is 66.2 s at 45.0^oC. What is its half-life (in s) at 65.0^oC?

The force constants for the diatomic molecules CO and HI are 1860 N/m and 320 N/m respectively.

Plot the potential energy curves for these two in a way that highlights their differences (i.e. on a single graph).

Calculate the frequency of motion for both molecules (does this result surprise you?).

Calculate the wavelength of light needed to excite these molecules from their vibrational ground states (v=0) to their vibrational first excited states (v=1).

10. Potassium oxalate is a monohydrate salt that forms colorless, odorless crystals. Oxalic acid is a diprotic acid with Ka1 = 5.4 x 10-2 and Ka2 = 5.3 x 10-5. (a) If 1.843 g potassium oxalate monohydrate is dissolved in enough water to make 100.0 mL of solution, what will be the pH of the solution? (b) What is the equilibrium concentration of the fully protonated oxalic acid? (c) Is this solution a buffer? Explain.

Calculate the pH for 0.80 M N(CH3)3, Kb=2.4x10^-7

Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Ka1 = 1.26 x 10–3; Ka2 = 5.6 x 10–6; Ka3 = 3.32 x 10–10) with 0.10 M NaOH. Indicate the volume needed to reach the first, second, and third equivalence points and the pH at the half equivalence points for the three titration regions.

A 1.500 Liter vessel is filled with 1.500 moles of hydrogen gas, and 2.500 mol of iodine gas to form hydrogen iodide gas at 448 oC. The reaction has an equilibrium constant of 53.5. What is the equilibrium molar concentration of all species?

5) A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution

a) before the addition of any LiOH.

b) after the addition of 30.0 mL of LiOH.

c) after the addition of 50.0 mL of LiOH.

d) after the addition of 66.67 mL of LiOH (this is the equivalence point).

e) after the addition of 75.0 mL of LiOH.

Please define each with credible references:

Pauli’s Exclusion Principle:

Aufbau Principle:

Hund’s Rule:

Periodic Trends

Atomic Size:

Ionization Energy:

Electron Affinity:

Metallic Character:

pH of salts

Determine if the following salts will raise, lower, or not change the pH of pure water when dissolved in the water.

a) NaCN

b) FeCl₃

c) HCOOH

d) K₂SO₄

e) K₃PO₄

f) SrCl₂

g) (CH₃)₂NH

h) Al(NO₃)₃

i) Li₂CO₃

j) KBr

k) Ca(NO₃)₂

l) NH₄Cl

m) KBrO₂

n) Zn(OH)₂

o) Ba(OCl)₂

p) CH₃NH₃Br

q) NaMnO₄

r) Li₂SO₃

s) BaI₂

t) SnBr₄