calculate the equilibrium concentration of H2CO3 and HCO3 in 1.0M Na2CO3 at 25 Celsius

Part1. Calculate the nuclear binding energy (in J) and the nuclear binding energy per nucleon of

(241.0568453 amu).

Part 2.

A freshly isolated sample of ⁹⁰Y was found to have an activity of 8.2 × 10⁵ disintegrations per minute at 1:00 p.m. on December 3, 2006. At 2:15 p.m. on December 17, 2006, its activity was measured again and found to be 2.2 × 10⁴ disintegrations per minute. Calculate the half-life of ⁹⁰Y.

Given 855cm^3 of a 0.00330M silver nitrate is mixed with 424cm^3 of a .0110M potassium chromate find,

a) balanced equation for both substances when placed in water

b) equation for the net ionic reaction

c) Ksp expression

d) concentration of all ions in solution after mixing but before any reaction takes place

1.    Write A for anti- addition or S for syn-addition to alkenes on the line provided for each of the following:

_______ Hydroxylation with cold Permanganate oxidation

---------------Catalytic hydrogenation

-------------Bromination

-----------------Chlorination

_______ Halohydrin formation

       ___ Hydroxylation with Osmium tetroxide

_______ Hydroboration/oxidation (Non-Markovnikov addn)

_______ Hydroxylation by acid -catalyzed epoxide hydrolysis

_______ Epoxidation with a peroxyacid

________Carbenes addition to yield cyclopropanes

_________ Ozonolysis in forming the molozonide

Briefly state the principle of a Faraday Cup detector for a mass spectrometer.

For each of the following sets of chemicals, predict their relative reactivity in the given type of reaction mechanism. List them in order (from least reactive to most reactive) and explain why (the one most significant cause for this trend of reactivity).

a) 1-chlorobutane vs 1-chloro-2-butene in S_N1

b) 2-chlorobutane vs 1-chloro-2-butene in S_N1

c) 1-chlorobutane vs 1-chloro-2-methylpropane in S_N2

The following reversible gas-phase reaction is carried out in a 10 L batch reactor.
A <->C -rA = CA – 0.5CC [mol/(L h)]
Determine the pressure, temperature, and gas phase composition (mole fractions) in the reactor after 1
hour of operating adiabatically given the following initial conditions and physical properties and the
assumption of ideal gas behavior:
P0 = 100 kPa, yA0 = 0.5, yC0 = 0.1, yinert=0.4, T0 = 500 K.
cpA = cpC = 10 J/mol K, cpinert = 5 J/mol K, HR(298K) = -20 kJ/mol C formed

What is the vapor pressure of a solution of 300 g of ethylene glycol, HOCH₂CH₂OH (mol wt = 62.1) and 200 g of water (a 60% solution by weight) at 100 ºC. The vapor pressure of pure water is 760 torr at 100 ºC (the boiling point of water).

1)A typical commercial antacid tablet contains 0.350 g of CaCO3 [MW=100.09 g/mol] as an active ingredient. How many moles of HCl could this tablet neutralize? 2)A student was analyzing an antacid tablet with a mass of 2.745 g. The student found that a 1.872 g sample of the tablet would neutralize 67.35 mL of stomach acid. Calculate how much stomach acid would be neutralized by the entire tablet. 3)A student determined that 29.43 mL of 0.132 M NaOH reacts with 25.0 mL of stomach acid. He dissolved a commercial tablet of antacid into 180 ml of stomach acid and then removed a 20.0 mL of the resulting solution. The Titration of this 20 mL sample took 9.56 mL of NaOH. Calculate volume of acid neutralized by antacid in the 200mL sample. 4) A 0.248 g sample of antacid containing an unknown amount of triprotic base Al(OH)3 [MW=78.00 g/mol] was reacted with 25.0 mL of 0.121 M HCl. The resulting solution was then titrated with 12.26 mL of 0.132M NaOH solution. Calculate the mass percent of Al(OH)3 in the antacid sample

Rotational spectroscopy observe what type of molecule? What is his energy range? Measured molecule properties.

vibrational spectroscopy observe what type of molecule? What is his energy range? Measured molecule properties.

A 25.0-mL solution of 0.100 M acetic acid is titrated with a 0.200 M KOH solution. Calculate the pH after the following additions of the KOH solution:

a) 0.0 mL b) 5.0 mL c) 10.0 mL d) 12.5 mL e) 15.0 mL

Question: A beaker with 1.40×10² mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 6.60 mL of a 0.430 M HClsolution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.

Please explain your steps. Thank you!

Hi!

I kep trying this question and can't get it right.

At a certain temperature, the equilibrium constant for the following chemical equation is 2.90. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.73 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.

SO2(g) + NO2(g) ----> SO3 (g) + NO (g)

Answer in mol NO2