Analyze how how efficiency can be just a function of the two temperatures for Carnot Cycle of ideal gas.

In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c).

(a) Calculate the pH when 0.029 moles of HCl are added to 1.000 liter of water.

(b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added?

(c) Calculate the pH when 0.029 moles of HCl are added to 1.000 liters of a buffer containing 0.396 M KH2PO4 and 0.201 M K2HPO4.

(d) The pH before the HCl was added is equal to 6.913. What is the difference between the pH before adding the HCl and after adding the HCl?

The reaction CH2Cl2 (g) --> CH4 (g) + CCl4 (g) has Kp = 1.33 at 400K. A 5.00L reaction vessel is evacuated, and 15.00 g of CH2Cl2 (l) is added to the flask. The CH2Cl2 (l) rapidly vaporizes and the reaction starts. a. What will be all of the partial pressures of the gases when equilibrium is reached? b. Sketch a graph showing the initial concentration of each gas and how they change as the mixture approaches equilibrium. Set-up your graph so that equilibrium is reacched two thirds of the way from the start to the end of the graph

Some measurements of the initial rate of a certain reaction are given in the table below.

Use this information to write a rate law for this reaction, and calculate the value of the rate constant.

Round your value for the rate constant to 3 significant figures

Also be sure your answer has the correct unit symbol.

Rate = k?

k = ?

Over what pH range(s) could valine be used as an effective buffer? Explain your answer, supporting it with what we have discussed about buffers and amino acids

The hydronium ion concentration of an aqueous solution of 0.497 M triethanolamine (a weak base with the formula C6H15O3N) is ... [H3O+] = _ M

The pOH of an aqueous solution of 0.462 M caffeine (a weak base with the formula C8H10N4O2) is .

What is the pH of a solution prepared by adding 1.46g of NaNO₂ to 143.00 mL of water? (Base Ionization Constant for NaNO₂ = 2.22E-11)

1. (9 pts) Consider a buffer solution composed of C6H5NH3+ and C6H5NH2. (Kb for the amine base is 3.9 x 10-10)

a. What is the optimum buffer range for this mixture?

b. What ratio of C6H5NH2 to C6H5NH3+ would be needed to buffer a solution at pH 4.10?

c. What is the pH of a solution containing 0.35 M C6H5NH3+ and 0.45 M C6H5NH2?

d. What is the pH after addition of 0.0015 mol of HBr to 20 mL of the solution in part c?

Nitric acid and magnesium hydroxide react to form magnesium nitrate and water

A) how many moles are in 83.1 ml of 1.581M nitric acid?

B) how many moles r in 54.3ml of 1.815M magnesium hydroxide?

C) what is the limiting reactant, and what is the theoretical yield of magnesium nitrate in gram?

D) if 2.831 g of mag. Nitrate r produced in the reaction what is the percent yield

A) For the following reaction, 4.22 grams of carbon (graphite) are allowed to react with 15.1 grams of oxygen gas. carbon (graphite) (s) + oxygen (g) carbon dioxide (g) What is the maximum amount of carbon dioxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

B) For the following reaction, 60.4 grams of iron(III) oxide are allowed to react with 24.7 grams of aluminum. iron(III) oxide (s) + aluminum (s) aluminum oxide (s) + iron (s) What is the maximum amount of aluminum oxide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams

Quantum numbers arise naturally from the mathematics used to describe the possible states of an electron in an atom. The four quantum numbers, the principal quantum number (n),(n), the angular momentum quantum number (?),(?), the magnetic quantum number (m?),(m?), and the spin quantum number (ms)(ms) have strict rules which govern the possible values.

Identify all allowable combinations of quantum numbers for an electron.

1. n=3, ?=-2, m? = -2, ms = +1/2

2. n=3, ?=2, m? = -2, ms = -1/2

3. n=5, ?=4, m? = -1, ms = -1/2

4. n=2, ?=0, m? = 0, ms =1

5. n=1, ?=1, m? = -1, ma = -1/2

6. n=4, ?=3 m? = 4, ms = -1/2

A buffer solution is composed of 1.723 g ofKH2PO4and 5.351 g of Na2HPO4 . ( ka for dihydrogen phosphate ion is 6.2x10^-8 .)

pH =  

Mass =  g

A-What is the pH of the buffer solution?

B-What mass of KH2Po4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a?

What would the pH of a solution containing 3.24g of an acid HX (Molar Mass of HX = 70.00 g/mol) after the addition of 1.49g of NaX? Assume no volume change to the solution after the addition of the NaX. (HX K_a = 1.30E-6)