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cerisehound374Lv1

6 Oct 2020

A hydrogen atom has a diameter of 1.06 x 10-10 m. The nucleus of the atom has a diameter of approximately 2.40 x 10-15 m.

a. For a scale model, represent the diameter of the hydrogen atom by the playing length of an American football field (100 yards = 300 ft) and determine the diameter of the nucleus in millimeters.

b. Find the ratio of the volume of the hydrogen atom to the volume of its nucleus.

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Francis VallesfinLv6

15 Nov 2020

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provided to determine AH rxn for the following reaction: urf (klimol) CH4(g) + 3 Cl2(g) â CHCI3() + 3 HCI(g) airrxn-? A)-151 kJ B)33SkJ C) +662kJ D) +117kJ E)-217 kJ A) 4.1 atm B) 5.0 atm c) 6.4 atm D)1.1 atm E) 2.3 atm kg) of the copper sample if the specific heat capacity of copper is 0 CH4(g) 75 CHCI3() -134 HCI(g) -92 8) What pressure will 14.0 g of CO exert in a 3.5 L container at 75 C? 9) A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 50.0Â°C, determine the mass (in .385 J/g C A) 226 kg B) 0.235 kg C)6.64 kg D) 119kg E)5.10 kg 10) Which of the following processes is exothermic? A) the ionization of a melting snow atom B) the breaking of a boiling of water bond C) the boiling of water D) the condensation of water E) All of the above processes are exothermic 11) Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. B)4.27 x 10-19J C) 2.34 x 10-19J D)6.45 x 10-19J E) 2.83 x 10-19J A)3.54 Ã 10-19J 12) Identify the color of a flame test for potassium D) yellow A) violet B) red C) white E) blue 13) Which of the following statements is TRUE? A) The emission spectrum of a particular element is always the same and can be used to identify the element. B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. C) The uncertainty principle states that we can never know both the exact location and speed of an electron. D) An orbital is the volume in which we are most likely to find an electron. E) All of the above are true. 14) Calculate the wavelength of an electron (m-9.11 x 10-28 g) moving at 3.66 Ã 106 m/s. A)1.99 x 10-10m B)5.03 x 10-10 m C) 1.81Ã10-10 m D)5.52 Ã 10-9 m E) 2.76 Ã 10-9 m 15) Which of the following quantum numbers describes the shape of an orbital? A) principal quantum number B) magnetic quantum number C) spin quantum number D) SchrÃ¶dinger quantum number E) angular momentum quantum number 16) Determine the energy change associated with the transition from n = 2 to n-5 in the hydrogen atom. A)-218Ã10-19J B)+654 Ã 10-19 J C) +4.58 x 10-19 J D)-1.53 x 10-19 J E) +3.76 Ã 10-19J 17) If two electrons in the same atom have the same value of I, they are A) in the same sublevel, but not necessarily in the same level. me level, but different sublevel. C) in the same orbital. D) in different levels and in different shaped orbitals. E) none of the above.

The equation Mg + HCl ï®MgCl2 + H2 can be balanced by _____.

A) Changing the coefficient of Mg to 2

B) Changing the coefficient of HCl to 2

C) Changing the coefficient of MgCl2 to 12 .

D) Changing MgCl2 to MgCl

E) Changing H2 to H

In the reaction below, how many molecules of water can be made from 38 molecules of C6H12O6?

C6H12O6 + 6O2 ï® 6H2O + 6CO2 A) 38
B) 6
C) 144

D) 228 E) 44

In the chemical reaction H2SO4 + 2NaOH ï®Na2SO4 + 2H2O, the coefficient of sodium sulfate is _____.
A) 0
B) 1

C) 2 D) 3 E) 4

H2CO3 ï®CO2 + H2O is an example of which type of reaction?

A) Substitution

B) Combination

C) Combustion

D) Decomposition

E) Formation

In the reaction H2 + F2 ï® 2 HF, which of the following is true?

A) H2 is reduced

B) H2 is the oxidizing agent

C) F2 is reduced

D) HF is called the reducing agent

E) HF is called the oxidizing agent

Page 1

Ascorbic acid (C6H8O6) acts as an antioxidant by being oxidized to _____. A) C6H8O6
B) C6H8O8
C) C4H9O7

D) C6H6O4 E) C6H6O6

During anaerobic metabolism pyruvic acid is converted to _____.

A) lactic acid

B) citric acid

C) oxalic acid

D) acetic acid

E) nitric acid

Reduction of CH3 = CH3 by hydrogen yields _____.

A) 2CH4

B) CH2 = CH2

C) CH3CHO

D) C2H6

E) CH3OH

Which of the following is not considered to be a form of reduction?

A) Gain of a hydrogen ion

B) Gain of electrons

C) Loss of an oxygen ion

D) Gain of negative charge

E) Gain of a sodium ion

Consider the reaction:
Au(s) + 3HNO3(aq) + 4HCl(aq) ï® HAuCl4(aq) + 3NO2(g) + 3H2O(l), how many Au atoms will react with 996 molecules of HCl?
A) 1992
B) 996
C) 498
D) 249
E) 336

Page 2

Oxidation of CH3CHO gives _____. A) CH3COOH

B) C2H6
C) C2H5OH D) H2C=CO E) CH3OH

Three moles of (NH4)2Fe(SO4)2Â·6H2O contains _____ moles of H2O.

A) 3

B) 6

C) 9

D) 12

E) 18

How many moles of hydrogen atoms are present in 27 grams of H2O?

A) Approximately one

B) Approximately one and a half

C) Approximately two

D) Approximately two and a half

E) Approximately three

Five
atoms of nitrogen?

A) 140.07 u

B) 28.014 u

C) 14.007 u

D) 280.14 u

E) 42.021 u

What is the molar mass of MgCO3?

A) 56.928 g/mol

B) 71.173 g/mol

C) 85.755 g/mol

D) 84.313 g/mol

E) 36.312 g/mol

moles of nitrogen molecules have a mass of 140.07 g. What is the mass of 10

Page 3

Consider the formation of ammonium chloride given by the equation:
NH3 + HCl ï® NH4Cl. How many grams of HCl would fully react with 76.43 moles of ammonia?
A) 1302
B) 2787
C) 2709
D) 4088
E) 4071

In the reaction 2P + 5Cl2 ï® 2PCl5, how many moles of atomic chlorine need to be reacted to form 525 g of PCl5?

A) B) C) D) E)

18. 1 Pa A)

B) C) D) E)

1.00 3.15 2.00 12.6 6.30

= _____ 1 atm
1 torr
1 J/s

1 N/m2 1 kJ/m

If a sample of gas has an initial pressure of 2.36 atm and an initial volume of 10.7 L, what is the final pressure if the volume is reduced to 4.09 L? Assume that the amount and the temperature of the gas remain constant.

A) 103 atm

B) 6.17 atm

C) 0.902 atm

D) 43.8 atm

E) 18.5 atm

A gas sample at 40Â°C has an initial volume of 40.0 L. What is its volume if the temperature is changed to 120Â°C? Assume that the pressure and the amount of the gas remain constant.

A) 1.99 L

B) 8.13 L

C) 50.2 L

D) 31.9 L

E) 123L

Page 4

Three moles of (NH4)2Fe(SO4)2Â·6H2O contains _____ moles of hydrogen atoms.

A) 4

B) 6

C) 20

D) 60

E) 100

How many moles of oxygen atoms would be present in 3.65 moles of Na2SO4?

A) 13.56

B) 3.65

C) 7.30

D) 10.95

E) 14.60

How many moles of NaCl are present in 20.0 g of NaCl?

A) 58.4

B) 1.01

C) 29.2

D) 0.342

E) 0. 0143

How many moles of oxygen atoms are present in one mol of (C2H5COO)2Ca?

A) 1

B) 2

C) 3

D) 4

E) 5

Codeine (C18H21NO3) is a painkiller. What is the molar mass of codeine? A) 195.60

B) 299.37 C) 227.30 D) 211.43 E) 313.35

Page 5

In the reaction H2SO4 + 2NaOH ï® Na2SO4 + 2H2O, the number of moles of H2O that can be produced from 10 moles of NaOH is _____.
A) 2
B) 3

C) 5 D) 10 E) 20

How many cal is 542.0 kJ? A) 129.5

B) 542.0 C) 2267 D) 542,100 E) 129,500

Which of the following is the correct definition for the specific heat of a particular substance?

A) The amount of heat released when one gram of the substance is heated.

B) The temperature change when one gram of the substance is burned.

C) The amount of substance in grams which when cooled by 1Â°C releases 1kJ of

energy.

D) The amount of heat released when one gram of a substance is cooled by 1Â°C.

E) The amount of heat absorbed when the temperature increases by 1Â°C

A specimen weighing 100.0 g is heated from 30.00Â°C to 63.30Â°C. If the quantity of heat transferred is 5834 cal, determine the specific heat of the specimen.

A) 17.25 cal/ gÂ·Â°C

B) 1.572 cal/ gÂ·Â°C

C) 12.75 cal/ gÂ·Â°C

D) 1.752 cal/ gÂ·Â°C

E) 1.257 cal/ gÂ·Â°C

What quantity of heat is transferred when a 250.0 g block of aluminum is heated from 25.00Â°C to 73.30Â°C? (Hint: The specific heat of aluminum = 0.2150 (cal/gÂ·Â°C).)

A) 56160 cal

B) 2596 cal

C) 1.110 cal

D) 1298 cal

E) 8986 cal

Page 6

How much heat is necessary to melt 70 g of ice (solid H2O) at 0Â°C? The heat of fusion of H2O is 79.9 cal/g.

A) 73 cal

B) 79 cal

C) 5500 cal

D) 1400 cal

E) 5600 cal

What is the process by which a substance forms vapor directly from the solid state without becoming a liquid?
A) Melting
B) Sublimation

C) Fusion
D) Condensation E) Vaporization

Which of the following statements is true for the bonding of atoms?

A) The energy of a compound is equal to the energies of the atoms which make up the

compound.

B) The energy of the individual atoms is lower than the energy of the compound.

C) The formation of a compound naturally, from individual atoms requires external

energy.

D) When a compound disintegrates there is a release of energy which equals the

difference in energy between individual atoms.

E) Individual atoms have higher amounts of energy than when in a compound.

What term is used to describe the strength of interactions between atoms in an ionic compound?

A) Bond energy

B) Lattice energy

C) Chemical energy

D) Crystal energy

E) Ionic energy

The reaction between sodium metal and HCl gives off heat. This type of reaction is called an _____ reaction.

A) isothermal

B) exothermic

C) endothermic

D) energy requiring

E) energy-less

Page 7

Which of the following is an endothermic reaction?

A) 2H2 + O2 ï® 2H2O + 135 kcal

B) H2 + F2 ï® 2HF + 130 kcal

C) CH4 + 2O2 ï® CO2 + 2H2O + 213 kcal

D) C2H4 + H2 ï® C2H6 + 137 kJ

E) 2SnCl2 + 33 kcal ï® Sn + SnCl4

Which of the following is true about gases?

A) They have a definite shape.

B) Their particles are in close contact with each other.

C) They have no definite volume.

D) They take the shape of the bottom of the container.

E) They have strong intermolecular interactions.

As
other and with the walls of their container. The force generated by gas particles divided by the area of the container walls yields_____.
A) volume
B) pressure
C) temperature
D) amount
E) density

If a sample of gas has an initial pressure of 4.83 atm, what is the initial volume if the pressure is increased to 10.0 atm and the volume is reduced to 10.0 L? Assume that the amount and the temperature of the gas remain constant.

A) 10.0 L

B) 20.7 L

C) 4.83 L

D) 483L

E) 0.207 L

A sample of gas has Pi = 0.50 atm, Vi = 9.5 L, and Ti = 290 K. What is the final volume

if Pf A) B) C) D) E)

= 0.75 atm and Tf = 350 K? 7.6 mL
7.6 cL
7,600 cL

7,600 mL 7,600 L

Experiment 1: Calculating Rate of Reaction

In this experiment you will calculate the rate of reaction of potassium iodide and hydrogen peroxide. The order of the reaction will also be determined.

Materials:

20 mL 3% Hydrogen peroxide, H₂O₂
15 mL Iodine-Potassium Iodide Solution, IKI (1% Iodine, 2% Potassium Iodide)
100 mL Beaker
10 mL Graduated cylinder
100 mL Graduated cylinder
250 mL Beaker
(2) 250 mL Erlenmeyer flasks
1-Hole Rubber stopper
2-Hole Rubber stopper
(2) 3 in. Rigid tubing pieces
(1) 6 in. Rigid tubing
6 Pipettes

Stopwatch
Permanent marker
Waste beaker (any volume)
*Access to graphing software
*Access to a computer
*24 in. Flexible tubing
*Water
*10 mL Distilled water

* You must provide

*You must cut this piece of tubing into two, 12 inch pieces. (if you have not already done so).

Procedure

Preparation of Apparatus

Set up apparatus as shown in Figure 2. To do this, begin by labeling the Erlenmeyer Flasks as 1 and 2. The reaction will take place in Flask 1.

Fill Flask 2 approximately three quarters of the way full with water.

Press the 2-hole rubber stopper into the top of Flask 2. Place one three in. piece and one six in. piece of rigid tubing into each hole of the rubber stopper. This should create an airtight system.

Place the one-hole stopper on Flask 1, and fit the remaining 3 in. piece of rigid tubing in the stopper hole.

Connect Flask 1 and Flask 2 with the two, 12 in flexible tubing pieces. One piece should connect Flask 1 to Flask 2, and the second piece should connect Flask 2 to the graduated cylinder. The tubing which connects Flask 2 to the graduated cylinder should be positioned low enough to be immersed in the water in Flask 2.

Figure 2: Apparatus set-up. Note this is a sample set-up and is not drawn to scale. Your specific equipment may vary slightly.

Part A: Preparation of Reactants

Pour five mL of the IKI solution into a 10 mL graduated cylinder.

Add five mL of distilled water to the graduated cylinder to bring the total volume to 10 mL. This is the 0.5% - 1.0% (diluted) IKI solution.

Pour 15 mL of 3% H₂O₂ solution into a 100 mL beaker.

Add five mL of distilled water to this beaker and mix with a stir rod. This is the 2.25% (diluted) H₂O₂ solution.

Part B: Performing the Reaction

Remove the stopper from Flask 1 and place five mL of the 3% (undiluted) H2O2 solution and 10 mL of the undiluted IKI solution provided into the flask. Immediately replace the stopper on the flask.
Note: At this point, you should select an extra beaker (any volume) from your lab kit to use as an supplemental collection container beaker for Step 6. You do not need to use the beaker yet, but keep it in close proximity.

Swirl Flask 1 until you observe a steady dripping of water going into the 10 mL graduated cylinder. This could take 3 - 5 minutes. Check for leaks in the tubing or system if water does not start rising up the plastic tubing coming from Flask 2 and traveling towards the graduated cylinder within one minute.

Stop swirling Flask 1 when you notice the steady flow of water droplets. When you stop, the water drop -rate will significantly decrease (to around one drop every 5 - 20 seconds) and could take a few minutes to stabilize. If a steady flow of drops of water does not occur within a few minutes, swirl Flask 1 for 1 more minute and check again. Repeat this process until there is a steady flow of drops of water after you have stopped swirling Flask 1.

Quickly empty liquid that has collected in the 10 mL graduated cylinder and replace the empty cylinder back under the flexible tubing.

Allow the flow of drops to become steady again. This could take 1 - 3 mL of water.

Start timing once the drop rate is steady and the volume of water collected is at a whole number (such as three mL). Record the time in Table 1 each time 2 mL of is water displaced. Continue taking data until you have at least 10 data points (20 mL displaced).
Note: Use the extra beaker (located in Part B: Step 1) to collect additional fluid when the volume of displaced water exceeds 10 mL.

Return the collected water from your 10 mL graduated cylinder to Flask 2. Ensure the seal is air tight.

Empty, clean and dry Flask 1 and the graduated cylinder.

Repeat Steps 1 - 8 for the following trial conditions: 5 mL 3% (undiluted) H₂O₂ mixed with 10 mL of 0.5%-1.0% IKI solution (placed in Flask 1); and, 5 mL of 2.25% H₂O₂ mixed with 10 mL of 1.0%-2.0% IKI solution (placed in Flask 1). Record the data in Table 2 and Table 3, respectively.
Note: Clean the graduated cylinder and extra collection beaker before it is used to measure any additional reagents for Trial 2 or Trial 3; and, before it is used for collecting the water from the reaction in the apparatus.

Use a graphing software program to make a graph of each trial. The graph should demonstrate the relationship formed between time vs. mL of water displaced.

Find and record the slope and the inverse slope for each trial.

Table 1: 10 mL Undiluted (1.0 -2.0%) IKI and 5 mL 3% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Table 2: 10 mL Diluted (0.5-1.0% IKI) and 5 mL 3% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Table 3: 10 mL Undiluted (1.0 -2.0%) IKI and 5 mL 2.25% H₂O₂
mL water displaced	Time (seconds)
2
4
6
6
8
10
12
14
16
18
20
22
Slope:
Inverse Slope:

Calculations

Post-Lab Questions

1. Determine the order of the KI in this reaction.

2. Determine the order of the H2O2 in this reaction.

3. Calculate the rate law constant.

4. What is the overall rate law?

5. When finding the order of H2O2, why was Trial 1 and Trial 3 used?

6. When finding the order of KI, why was Trial 1 and Trial 2 used?

7. Research and identify some alternative catalysts that could be used to accelerate the decomposition of hydrogen peroxide. Evaluate these catalysts and determine which option is

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