At 700 K acetaldehyde decomposes in the gas phase to methane and carbon monoxide. The reaction is:
CH3CHO(g)→CH4(g)+CO(g)
A sample of CH3CHO is heated to 700 K and the pressure is measured as 0.27 atm before any reaction takes place. The kinetics of the reaction are then followed by measurements of total pressure and these data are obtained:

Find total pressure after 1.47×10⁴ s .

5. Consider the combustion of carbon monoxide (CO) in oxygen gas: 2CO(g) + O₂(g) → 2CO₂(g)

A. Calculate the number of moles of CO₂ produced if 2.86 moles of CO is reacted with excess oxygen._______ moles CO_2.

B. Determine the moles of oxygen required to react with the CO._______ moles O₂

6. Consider the following balanced chemical equation: C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l)

a. How many moles of CO₂ form when 1.73 moles of C₂H₅OH react? ______ moles CO₂

b. How many moles of H₂O form from the reaction of 1.73 moles of C₂H₅OH?_____ moles H₂O

c. How many moles of CO₂ form when 1.73 moles of H₂O form? _____moles CO₂

d. How many molecules of CO₂ form when 1.73 moles of H₂O form? _____ × 10 ^? molecules CO₂

7.   How much oxygen (in grams) will form from 15.2 mg of N₂O₅?

2N₂O₅(s) → 4NO₂(g) + O₂(g)---------> × 10^?g O₂

8. How much oxygen (in grams) will form from 65.2 g of N₂O₅?

2N₂O₅(s) → 4NO₂(g) + O₂(g) ---------> × 10^? g O₂

A method used by the Environmental Protection Agency (EPA) for determining the concentration of ozone in air is to pass the air sample through a "bubbler" containing sodium iodide, which removes the ozone according to the following equation: O3(g)+2NaI(aq)+H2O(l)→O2(g)+I2(s)+2NaOH(aq)

Part A) How many moles of sodium iodide are needed to remove 5.95×10⁻⁶ mol O3?

Part B) How many grams of sodium iodide are needed to remove 2.1 mg of O3?

The proton NMR spectrum for a compound with the formula C7H14O is shown below along with carbon-13 spectral data in tabular form. (It may be necessary to expand (zoom) some of the 1H signals to view spin-spin splitting details.)

This compound exhibits strong infrared absorption at 1717 cm^-1, but the 1500-1650 cm^-1 region is empty.

How would the following experimental errors affect your experimental results while separating the components of a counterfeit pharmaceutical (yield, purity or both) and explain why. A) you failed to dry the product completely. B)you used enough water to recrystallise phenacetin, however your Unknown was acetanilide. C)in experiment 1, you didn't extract all of the aspirin from DCM solution.

What is the rate constant of a first-order reaction that takes 127 seconds for the reactant concentration to drop to half of its initial value?

Determine the w/w% of chloride in unknown.

6.4923g of AgNO3 is dissolved in 500mL of water producing a 0.076438M solution.

1.4838g of CaCl2 is dissolved into 250mL of water producing a 5.3479x10^(-2)M solution.

10.00mL pipette is calibrated to 9.927mL

25.00mL pipette is calibrated to 25.163mL

Each of th five flasks contains 25.163mL of the CaCl2 solution

For the unknown each of the five flasks contains 25.163mL

Titrations

UNKNOWN

The first titrations of each round were rough titrations and should not be included

Consider the titration of a 23.0 mL sample of 0.120 molL−1 RbOH with 0.110 molL−1 HCl. Determine each quantity:

Part A

the volume of added acid required to reach the equivalence point

Part B

the pH at 5.7 mL of added acid

Express your answer using two decimal places.

Part C

the pH after adding 6.0 mL of acid beyond the equivalence point

Express your answer using two decimal places.

Describe an example of the complimentary principle of matter. This is the concept that matter has both particle and wave properties.

Hydrogen produced from a hydrolysis reaction was collected over water and the following data was compiled.

Total volume of H2(g): 96.62 mL

Temp: 28.0C

Bariometric Pressure: 7.40x10^2 mmHg

Vapor pressure of water at 28C: 28.5 mmHg

Calculate the moles of hydrogen gas produced by the reaction.

1.0 gram samples of solutes A,B, and C are dissolved in 10.00 g of water to give three separate solutions. Use the information below to calculate the molecular mass of A, B, and C. Determine the molecular formula of solution B. Assume all solutes are nonvolatile and nonelectrolytes. 1. Solute A has a vapor pressure of 16.9 torr at 20 degrees C. The Vapor pressure of water at 20 degrees C si 17.5 torr. Calculate Molecular mass. 2. Solute B freezes at -1.03 degrees C and has an analysis of 40% Carbon, 53.6% Oxygen, and 6.7% Hydrogen. The Kf (constant of Freezingpoint) for water is 1.86. What is the moleuclar mass and molecular formula? 3. Solute C has an osmotic pressure of 1.6 atm at 25 degrees C. What is the molecular mass of this substance?

Consider the reaction:

H2(g)+I2(g)⇌2HI(g)

A reaction mixture in a 3.65 L flask at a certain temperature initially contains 0.764 g H2 and 97.0 g I2. At equilibrium, the flask contains 90.5 g HI.

Calculate the equilibrium constant (Kc) for the reaction at this temperature.

Kc = ?

Metals often form several cations with different charges. Cerium, for example, forms Ce3+ and Ce4+ ions, and thallium forms Tl+ and Tl3+ ions. Cerium and thallium ions react as follows:

2Ce4+(aq)+Tl+(aq)→2Ce3+(aq)+Tl3+(aq)

This reaction is very slow and is thought to occur in a single elementary step. The reaction is catalyzed by the addition of Mn2+(aq) according to the following mechanism:

Ce4+(aq)+Mn2+(aq)Ce4+(aq)+Mn3+(aq)Mn4+(aq)+Tl+(aq)→→ →Ce3+(aq)+Mn3+(aq)Ce3+(aq)+Mn4+(aq)Mn2+(aq)+Tl3+(aq)

Part A

What is the rate law for the uncatalyzed reaction?

What is the rate law for the uncatalyzed reaction?

The barrier to C-C bond rotation in bromoethane is 15 kJ/mol. What energy can you assign to an H-Br eclipsing interaction?
Use strain energy increments from the table below in your calculation.

(Specify units, kJ/mol; Calculate to nearest 0.1 energy units)

1. Select the statement that is NOT true about venting during an extraction.

A.The separatory funnel stem should not be pointed towards any person while venting.

B. The stopper must be held in place while venting.

C.The stopper must be held in place while venting.

D.The separatory funnel must be inverted before venting.

2. Select the general rule that is true about performing an extraction.

A. The top layer of the extraction contains the desired product.

B. All liquid layers should be saved until it is known which layer contains the desired product.

C. To avoid the formation of an emulsion, the bottom liquid layer should be separated from the top layer as quickly as possible.

D. During an extraction, the separatory funnel should never be inverted more than 10 times.

3. An emulsion forms during an extraction. Select the best course of action to quickly break the emulsion.

A. Shake the separatory funnel vigorously.

B. Dispose of the emulsion and restart the experiment.

C.Allow the emulsion to sit for 1–2 hours.

D. Add sodium chloride.