Describe one example of a property (and give one equation) of electromagnetic radiation that is particle like.

A flask containing pure NO₂ was heated to 1250K, a temperature at which the Kpvalue for the decomposition of NO2 is 177.

2 NO₂(g) <---------> 2 NO(g) + O₂(g)

Starting with pure NO₂ , the flask is heated and he partial pressure of O2 at equlibrium is 0.133 am. Calculate the partial pressures of NO and NO₂ at equlibrium and the total pressure in the flask at equlibrium.

P_NO ____________________atm

P_NO2____________________atm

P_total____________________atm

14: An electron in hydrogen atom at the energy level n = 7 undergo a transition to level n = 3: Find the frequency and the energy of the emitted photon.

15: An electron jumps from higher energy level to the first energy level with an energy difference of 2.04375 x 10^-18 J. find the initial energy level. Show your calculations,

16: A: What will be the speed of an electron at 4 th energy level? Suppose the electron has a wavelength of 97.3 nm Given Mass of electron is 9.11 x 10^-31 kg. Use de Broglie’s theory.

What is the maximum number of electrons in an atom that can have the following quantum numbers?

(a) n = 4, ms = -1/2

____

(b) n = 5, l = 3

____

(c) n = 6, l = 3, ml = -2

____

(d) n = 2, l = 1, ml = -1, ms = +1/2

____

A)An exactly 500 gram iron ore sample was determined to contain 242 grams of iron. What is the mass percent of iron in the ore?

B) What are the coeffieceints for the following properly balaned reaction-

__Sodium phosphate reacts with___barium nitrate to from ___sodium nitrate and ____barium phosphate

C) What mass of iron is present in a 6.03 gram sample of iron (II) chloride?

Indicate the concentration of each ion present in the solution formed by mixing the following. (Assume that the volumes are additive.)

(a) 30 mL of 0.100 M HCl and 10.0 mL of 0.520 M HCl

H+ _____M

Cl-______ M

(b) 15.0 mL of 0.294 M Na2SO4 and 28.2 mL of 0.200 M KCl

Na+______ M

K+______ M

SO42-______ M

Cl-______ M

(c) 3.50 g of NaCl in 59.3 mL of 0.439 M CaCl2 solution

Na+______ M

Ca2+______ M

Cl-______ M

Limiting Reactions Question #11

Part a.

For the following reaction, 0.289 moles of hydrochloric acid are mixed with 0.562 moles of oxygen gas.

Hydrochloric acid (aq) + oxygen (g) = water (l) + chlorine (g)

What is the FORMULA for the limiting reagent   ________________ and what is the maximum amount of water that can be produces? _____________moles

Part b.

For the following reaction, 9.80 grams of butane (C4H10) are allowed to react with 19.0 grams of oxygen gas.

Butane (C4H10)(g) + oxygen (g) = carbon dioxide (g) + water

What is the maximum amount of carbon dioxide that can be formed? ______________grams

What is the FORMULA for the limiting reagent ______________ and what amount of excess reagent remains after the reaction is complete? _______________grams

Adult hemoglobin (iron-containing protein) can carry up to four oxygen molecules per hemoglobin molecule, with the addition of oxygen proceeding in a step-wise fashion. For the third step, the value of the equilibrium constant is Keq=5.86 x 10^-4 although the reaction has a (delta Hº) value of -2.9 kj/mol (Remember that the system is not at room temperature).

Heme-Fe^2+ -(O2)2 + O2 <----> Heme-Fe^2+ -(O2)3

Keq=5.86 x 10^-4

(a) calculate delta Gº for this process.

(b)From the information provided, calculate the value of delta Sº for this process.

(c) Compare the value of delta Sº and delta Hº for this process and determine if the oxygenation of hemoglobin at this step is enthaly-driven or entropy-driven when this reaction is spontaneous. Explain your reasoning in a sentence or two.

1 Write a balanced equilibrium equation and equilibrium constant expression for the dissolution of Ca(OH)2(s).

2. If a compound is only slightly soluble, will the equilibrium lie “to the left” or “to the right” if the equation is written with solid on the left and the ions on the right?

3. Will the equilibrium constant (Ksp) be large or small for the reaction in question number 2?

consider a 1.00 M solution of a weak acid, HA. The pH of the solution is found to be 3.85. A) calculate the [H3O+] in the solution. This would be the equilibrium concentration of H3O+ in the solution. B) write out an ICE table as before. Here, we don’t know the numerical value of Ka but we know the [H3O+] at equilibrium which you should see from your ICE table easily relates to the value of “x” in your table and knowing “x” from [H3O+], one can easily determine the other equilibrium concentrations of all species and solve for value of Ka.

C) [H3O+] = __________________

1) How many atoms are there in 51.3 g of barium chloride (BaCl2)?
2) How many moles of carbon monoxide (CO) are in 29.3 g of the compound?

3) What is the formula for copper(II) phosphate? Capitalization and punctuation count?

4) How many atoms of phosphorus are in 2.90 mol of copper(II) phosphate?

5) How many moles of N are in 0.191 g of N2O?

6) A sample of C3H8 has 7.68 × 1024 H atoms. How many carbon atoms does the sample contain? What is the total mass of the sample?

7) Calculate the percent composition by mass of each element in Al(OH)3. Use at least three significant figures.

% Al= ?,   % O=?   ,   % H =?

8) What is the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass?

                HCO (Insert subscripts as needed.)

9) A compound with the empirical formula CH2 has a molar mass of 98 g/mol. What is the molecular formula for this compound?

Kinetic Study of an Iodine Clock Reaction.

Flask A contains 5.00 mL of 6 M HCl (density 1.11 g/mL). Flask B contains 5.00 mL of the same 6M HCl solution used in flask A, 2.00 mL of ethyl acetate (density 0.893 g/mL), and 3.00 mL of water (density 1.00 g/mL). Flask A was titrated with 1.00 M NaOH, and it required 31.95 mL to reach a phenolphthalein end point. Flask B was sealed and allowed to sit for 7 days to allow the system to reach equilibrium. At the end of the 7 day period, flask B was titrated with 1.00 M NaOH, and it required 42.75 mL of NaOH solution to reach a phenolphthalein end point.
Using the information above answer the following questions for the system outlined below.
ethyl acetate + water <--> ethyl alcohol + acetic acid

1-Based on the titration information for flask A, determine the number of moles of HCl in 5.00 mL of the 6 M HCl solution used for the experiment. Note that the concentration of the HCl solution is approximately 6M, and the actual concentration may be slightly higher or lower. Do not include units in your answer.

2-Calculate the moles of water in a 5.00 sample of the 6M HCl solution used for the experiment. Do not include units in your answer.

3-Determine the initial moles of water in flask B immediately after mixing. Do not include units in your answer.

4-Determine the initial moles of ethyl acetate in flask B immediately after mixing. Do not include units with your answer.

5-Determine the moles of acetic acid in flask B at equilibrium based on the titration data for flask B. Note that the HCl that was added to the flask is still present at equilibrium. Do not include units in your answer.

6-Using the moles of acetic acid at equilibrium, the stoichiometry of the reaction, and the initial number of moles of water, determine the moles of water at equilibrium. Do not include units with your answer.

7-Using the moles of acetic acid at equilibrium, the stoichiometry of the reaction, and the initial number of moles of ethyl acetate, determine the moles of ethyl acetate at equilibrium. Do not include units with your answer.

8-Calculate the equilibrium constant for the system.

The value of Ka in water at 25 °C for propionic acid (C2H5CO2H) is 3.4 x 10-5 M. What is the pH of a 0.020 M aqueous solution of propionic acid?

how the leaving group affect the behavior of the alkyl halide in mixture of NaI/ Acetone and in mixture of AgNO3/ Ethanol?

2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without a significant pH change. It is governed by the concentrations of the conjugate acid and base forms of the buffer. A 0.5 M buffer will require five times as much acid or base as a 0.1 M buffer for given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity of acid or base is added. In the laboratory you will carry out some stepwise additions of acid or base and measure the resulting pH values.

Starting with 60 mL of 0.50 M phosphate buffer, pH=6.83, you add 1.7 mL of 1.00 M HCl. Using the Henderson-Hasselbalch equation with pK2 for phosphate of 6.64 calculate the following values to complete the ICE table.

What is the composition of the buffer to begin with, both in terms of the concentration and the molar quantity of the two major phosphate species? (Units required.)

What is the molar quantity of H3O+ added as HCl, and final molar quantity of HPO and H2PO4- at equilibrium?

What is the new HPO42-/H2PO4- ratio, and the new pH of the solution?(Note: you can use the molar ratio rather than the concentration ratio because both species are in the same volume.)

Now take another 60 mL of the 0.50 M pH 6.83 buffer and add 3.7 mL of 1.00 M NaOH. Using steps similar to those above, calculate the new pH of the solution.