CH110 Chapter Notes - Chapter 5: Pennsylvania Route 100, Systematic Chaos, Molar Mass

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15 Dec 2016

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Fill and assume the shape of their containers. Small amount of one + large amount of another. Large amount of one + large amount of another. Are less likely to collide with each other. P = pressure (pa = kg m-1s-1. F = force (n = kg m s-2) Si unit for pressure is the pascal (pa); si unit for force is the newton (n) It is difficult to measure total force exerted by gas molecules. Pressure is a measure of the force a gas exerts on a surface. When a moving object collides with any surface it exerts a force and therefore pressure. When a particle collides with the contain wall, it exerts a force. All the collisions occurring at any instant make up the observed pressure. The more particles there are the more frequent the collisions are will the wall and therefore greater the pressure.

Related Questions

i need answers of all the 12 questions. plz provide steps as well

A mixture of H_2(g) and NH_3(g) has a volume of 139.0 cm^3 at 0.00 degree C and 1 atm. The mixture is cooled to the temperature of liquid nitrogen, at which ammonia freezes out and the remaining gas is removed from the vessel. Upon warming the vessel to 0.00 degree C and 1 atm, the volume is 77.4 cm^3. Calculate the mole fraction of NH_3 in the original mixture. A vessel contains 1.15 g of H_2O(I) in equilibrium with vapor at 30 degree C. At this temperature, the vapor pressure of H_2O is 31.82 torr. What will the volume be when all the water evaporates at this temperature? A rigid vessel of volume 0.400 m^3 containing H_2 at 21.25 degree C and a pressure of 715 times 10^3 Pa is connected to a second rigid vessel of volume 0.750 m^3 containing Ar at 30.15 degree C at a pressure of 203 times 10^3 Pa. A valve separating the vessels is opened and both are cooled to a temperature of 12.2 degree C. What is the final pressure in the vessels? An electric heater is immersed in a flask containing 150 g of ethanol and a current of 1.12 A is applied from a 12.5 V power supply for 172 s. Estimate the rise in the temperature of ethanol. Consider heating 1 kg of H_2O (i) by 10 degree C using each of the following methods a. Heat with a mechanical eggbeater that is powered by a 1-kg mass on a rope over a pully. How far does the mass have to descent in the earth's gravitational field to supply enough work? b. Make a charcoal fire. How much charcoal (graphite) must you burn? A homeowner uses 4.00 times 10^3 m^3 of methane (at 1.00 atm and 20 degree C) in a year to heat a home. How many grams of methane are used during this time period to heat the home? Consider a sample of a perfect gas whose temperature is -33.0 degree C and volume is 0.0250L. What temperature is required to change the volume to 66.9 cm^3? Hydrogen gas is used in weather balloons because it is less expensive than helium. Assume that 5.57 g of H_2 is used to fill a weather balloon to an initial volume of 67 L at 1.04 atm. If the balloon rises to an altitude where the pressure is 0.047 atm, what is the new volume? Assume that the temperature remains constant. The atmospheric surface pressure on Venus is 90 bar and is composed of 96% CO_2 and approximately 4% various other gases. Given a surface temperature of 730K, what is the mass of CO_2 present per cubic centimeter at the surface? A sample of propane (C_3H_8) is placed in a closed vessel together with an amount of O_2 that is 2.15 times the amount needed to completely oxidize the propane to CO_2 and H_2O at constant temperature. Calculate the mole fraction of each component in the resulting mixture after oxidation, assuming that the H_2O is present as a gas An initial step in the biosynthesis of glucose C_6H_12O_6 is the carboxylation of pyruvic acid CH_3COCOOH(s) to form oxaloacetic acid HOOCCOCH_2COOH: CH_3COCOOH(s) + CO_2(g) rightarrow HOOCCOCH_2COOH(s) What volume of CO_2 is required to produced 1.10 g of glucose? Assume p = 1.00 atm and T = 298 K. In an experiment to measure the molar mass of a gas, 250 cm^3 of the gas was confined to a glass vessel. The pressure was 152 torr at 298 K and the mass of the gas was 33.5 mg. What is the molar mass of the gas?

WORD BANK:

Atomic solids

Body-centered cubic

Boiling point

Condensation

Covalent atomic solids

Crystal lattice

Crystalline solids

Distillate

Distillation

Dynamic equilibrium

Evaporation

Face-centered cubic

Freezing

Freezing point

Ionic solids

Intramolecular

Interionic forces

Intermolecular forces

Liquid State

Macromolecule

Melting

Melting point

Metallic atomic solids

Molar heat of fusion

Molar heat of vaporization

Molecular solids

Non-bonding atomic solids

Non-crystalline (amorphous) solids

Properties of Liquids

Properties of Solids

Simple cubic

Solid State

Sublimation

Surface tension

Surfactants

Vapor pressure

Vaporization

Viscosity

Wetting action

Use the Vocabulary words above to complete the following sentences words can be used more than once, some words are not be used.

d. The molecules of a ________ are in constant motion. e. The __________ of a liquid is related to the shape of the molecules that make up the liquid. f. The force of attraction that causes the surface of a liquid to contract and form a âbeadâ or spherical drop is called? _________ _______ g. Chemical that reduce surface tension are called? __________ h. A liquids ability to spread out evenly over a surface as a thin film is called itâs? _________ _______ i. ____________ is the process by which molecules of a liquid break away and go into the gas phase. j. When the molecules of a volatile liquid jump to gas phase it is called _________. k. The reverse of evaporation (the conversion of a vapor to a liquid) is called? _________ l. When the rate at which the water is evaporating is equal to the rate at which the water vapor is condensing, you have established a __________ _________. m. ________ _______ is the partial pressure of a gas in dynamic equilibrium with its liquid. n. ________ _______ is when the vapor pressure equals the atmospheric pressure. o. Boiling point can be used to purify a solution of two or more substances by ________. p. The condensed vapor sample is called the? ________ q. The exact quantity of heat required to vaporize 1 mole of a liquid at constant pressure and temperature is called the ________ ________ ___ __________. r. In ________________ __________ the particles do not have a definite or regular order (there is no repeating pattern throughout the solid). s. In ____________ __________, the particles are arranged in regular, systematic patterns called a ________ _________. t. The three different types of crystal lattices based on the cube are? ________ ______, _____________ ______, and ___________, ________. u. The three types of atomic solids include _________ _____, ___________ ______, and __________ ________.

Decomposition of Malachite

Here is what Malachite is Made Out Of

Malachite is a famous and very popular semi-precious stone. Its banded light and dark green bands are one-of-a-kind, and give it a unique ornamental quality unlike that of any other stone. The light and dark green bands are so distinctive that malachite may be one of the most easily recognized minerals by the general public. Malachite is popular in jewelry, especially Native American southwestern jewelry. The stones inlayed in silver make a nice alternative to traditional turquoise jewelry.

Malachite is a form of copper carbonate with the molecular formula Cu₂CO₃(OH)₂. When heated to around 200 ï¿½C, malachite decomposes into copper (II) oxide (CuO) and other products.

Reaction Stoichiometry

The Law of Conservation of Mass states that matter can neither be created nor destroyed. Therefore, the number of atoms of each element on the reactants side must be same as the number of atoms on the products side. This quantitative study of chemical reactions is called stoichiometry. The substances in a balanced reaction are related to each other by stoichiometric molar ratios. For example, magnesium reacts with hydrochloric acid in a 1:2 stoichiometric ratio in the balanced equation below.

Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g)

The molar ratios can be used as conversion factors to find the amount (in moles) of one substance given the amount of another. For example, given the number of moles of HCl, the amount of MgCl₂ can be determined as shown below.

nMgCl2=nHCl x (1mol MgCl2) / (2mol HCL)

The molar ratios are used to determine the amount in moles. However, the amount of reactant or product is often measured in grams. Mass can be converted to moles and vice versa as shown below.

n = m / (MM)

m = n x MM

where n is the number of moles, m is the mass of the product in g, and MM is its molar mass in g/mol.

To observe the Law of Conservation of Mass, you can perform different types of chemical reactions. For example, you can use a decomposition reaction to observe one compound being broken down into two or more elements or new compounds. For this reaction to take place, you must break existing bonds within the starting compound. Different sources of energy such as heat, light, or electricity may be used. Through a decomposition reaction, you can observe that the atoms in the original compound are not destroyed but are rearranged to form simpler substances, such as elements or compounds.

About This Lab

In this lab, you will test if the relationship between malachite and copper (II) oxide is stoichiometric. To do this, you will heat a known mass of malachite to produce copper (II) oxide. You will then compare the amount of copper (II) oxide obtained experimentally with the amount of copper (II) oxide expected from the balanced equation for the decomposition reaction.

1.Take a crucible from the Containers shelf and place it on the workbench.

2.Take a balance from the Instruments shelf and place it on the workbench.

3.Move the crucible onto the balance. Record the mass of the empty crucible to the nearest 0.001g in your Lab Notes.

4.Move the crucible onto the workbench.

5.Take copper (II) carbonate hydroxide from the Materials shelf and add 10 g to the crucible.

6.Move the crucible onto the balance and record the mass of the crucible containing copper (II) carbonate hydroxide in your Lab Notes.

7.Take a Bunsen burner from the Instruments shelf and place it on the workbench.

8.Move the crucible onto the Bunsen burner.

9.Double-click on the crucible to open its properties. Select Show Contents and click OK. This gives you a cut-away view of the crucible's contents.

10.Turn the Bunsen burner on to low flame by clicking the knob at the bottom once. Clicking multiple times will increase the intensity of the flame until it is turned off.

11.Watch the crucible until the malachite fully decomposes. You will see a distinct color change.

12.Move the crucible onto the workbench to cool.

13.Turn off your Bunsen burner.

14.Weigh the crucible with its contents and record the mass to the nearest 0.001 g in your Lab Notes.

Clear your station.

Lab Notes:

Numbers below refer to numbers in the above âAbout this Labâ

3. Empty crucible = 88 g

5. Added 10 g of Copper (II) carbonate hydroxide to crucible

6. Crucible with Copper (II) carbonate hydroxide = 98 g

11. to Black

14. after heating crucible with its contents = 95.195

Questions I have answered:

How many grams of malachite did you add to the crucible? 10g

How many grams of product were in the crucible after heating? 7.195

By how much did the mass of the crucible's contents change after heating? -2.805

The molar mass of malachite is 221.1 g/mol. How many moles of malachite were present before the reaction? 0.04523 mol

The product remaining in the crucible after heating is copper (II) oxide. The molar mass of copper (II) oxide is 79.55 g/mol. How many moles of copper (II) oxide were produced during the reaction?

0.0945 mol

Please answer the following:

Q1 a. Which of the following represents the balanced chemical equation for this reaction?

Cu2CO3(OH)2=2CuO+H2O

Cu2CO3(OH)2=CuO+CO2

Cu2CO3(OH)2=2CuO+H2O+CO2

Cu2CO3(OH)2=CuO+H2O+CO2

b. Based on the number of moles of malachite that you started with, how many grams of water were produced? The molar mass of water is 18.0153 g/mol. Choose the closest answer.

1.815 g 0.8148 g 1.630 g 1.982 g

c. Based on the number of moles of malachite that you started with, how many moles of CO₂were produced? Choose the closest answer.

1.000 mol 0.04523 mol 0.9000 mol 0.09045 mol

d. Based on the number of moles of malachite that you started with, how many grams of CO₂were produced? The molar mass of CO₂ is 44.01 g/mol. Choose the closest answer.

1.991 g 0.4401 g 0.04523 g 3.981 g

Q2a. Based on the number of grams of CO₂ and H₂O produced during the reaction, does this compensate for the observed loss of mass?

A. No, because this violates the law of conservation of mass

B. yes, this compensates for the mass lost in the reaction

C. No, because more copper oxide was produced

D. No because mass is conserved

b. You observed that the products in the crucible weigh less than the reactants that you added. How is this possible?

A. Mass was lost due to experimental error

B. The Malachite absorbed CO2 from the air

C. CO2 and H2O were released as gases

D. Mass was converted to energy

c. What kind of a reaction took place upon heating?

A. decomposition

B. single displacement

C. synthesis

D. Double displacement

d. Baking soda is used as a leavening agent in baking. When heated, baking soda undergoes a decomposition reaction to form carbon dioxide. Given the data below, which of the following reactions occurs during baking? The molar mass of baking soda is 84.007 g/mol and the molar mass of carbon dioxide is 44.01 g/mol.

Mass of empty crucible (g) = 55.000

mass of crucible with baking soda (g) = 57.000

mass of crucible and contents after the reaction (g) =56.260

A. 2NaHCO3= 2Na+2CO2 +H2O

B. 2NaHCO3 = Na2O + 2CO2 +H2O

C. NaHCO3 = NaOH +CO2

D. 2NaHCO3 = Na2CO3 + CO2 +H2O

CH110 Chapter Notes - Chapter 5: Pennsylvania Route 100, Systematic Chaos, Molar Mass

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