week 33 chemistry

Week 33 ChemistryGas Laws

Warm Up: 4 Minutes

You should be working SILENTLYStay in your own seat

If the pressure of a tire is over 35 psi, it is likely to explode. If the initial pressure of a tire is 32.5 psi at 15 ºC, calculate the new pressure at 40 ºC.

Is the tire likely to explode at 40 ºC?

Write the Learning Target

This is the passing rate

How to improve your grade

Turn in missing assignments (this is the biggest issue right now)

Make up Missed Exams Come to tutorials for extra help

Agenda

Warm Up: 7 Minutes Combined Gas Law Video: 15 Minutes Guided Practice: 13 Minutes Independent Practice: 15 Minutes Closing: 3 Minutes

Combined Gas Law Video1. Go to shschem.weebly.com (our class

website)Bookmark this if you haven’t done so already!!!

2. Hover over my page:Mr. Ghosh Video Lessons

3. Watch video for April 284. Take notes on your handout

Let’s Review our Gas Laws

V VT T

P1V1 = P2V2

G. Lussac’s Law

Boyle’s Law

Charles Law

Putting them all together…

P1V 1n1T1

=P2V 2n2T 2

This is the

Combined Gas Law

# of Moles

Problem Solving Tip Begin all problems using the Combined Gas Law If any variables (P, V, n, or T) are not present,

delete them from both sides of the equation Substitute and solve using remaining values

Example: Problem has Pressure and Temperature, but no Volume or Moles

Example 1The initial pressure, temperature, and volume of a car tire are 33 psi, 25 ºC, and 4.8 L. If the temperature outside rises to 35 ºC and the volume expands to 5.0 L, what is the new pressure inside the tire?

Example 23.2 moles of gas have a volume of 800.0 mL at -23 ºC. How many moles of gas would be present in 675.0 mL at 227.0 ºC?

Guided Practice

Take 13 seconds to study the problem. When Mr. Ghosh indicates that you can talk,

take 48 seconds to work the problem with your teammates.

When Mr. Ghosh says SWAG, be ready to share and explain your answers.

Guided Practice #1A toy balloon contains 3 moles of gas at an internal pressure of 1.05 atm and a volume of 5.0 L. If the initial temperature of the balloon is 20 ºC, what will the volume of the balloon be if it rises to an altitude where the pressure is 0.65 atm and the temperature is -15 ºC?

7.11 L

Guided Practice #2A small research submarine contains gas with a volume of 1.2 x 105 L at a pressure of 1.0 atm and a temperature of 15 ºC. Assuming the number of moles remains constant, the submarine descends to a depth where the new volume is 767 L and the temperature is 3 ºC. What is the new pressure on the gas?

150 atm

Guided Practice #3If I initially have 4.0 L of a gas at a temperature of 38 ºC, what will the temperature be if I increase the volume to 5.0 L?

Independent Practice

Its time to see if you truly understand the Combined Gas

Law. ..

Closing

Which law relates P and V?

Which law relates V and T? Which law relates P and T? Which law relates P, V, n, and T?

Warm Up: 4 Minutes

The initial pressure, volume, and temperature a gas are 1 atm, 3.4 L, and 27 ºC. If the pressure increases to 3.2 atm, and the temperature rises to 79 ºC, what is the new volume?

Agenda

Warm Up: 7 Minutes Ideal Gas Law Video: 15 Minutes Guided Practice: 13 Minutes Independent Practice: 15 Minutes Closing: 3 Minutes

Ideal Gas Law Video1. Go to shschem.weebly.com (our class

Ideal Gas

Perfect gases under perfect conditions

IDEAL GAS LAWDESCRIBING THE BEHAVIOR OF IDEAL GASES

PV = nRTP = pressureV = volume in LITERSn = molesR = gas constantT = temperature in KELVIN

RKmolatmL

08206.0Kmol

kPaL314.8

KmolmmHgL

Example 1What is the volume of 0.25 moles of oxygen gas at 250 K and 360 mmHg? Kmol

kPaL314.8

KmolmmHgL

KmolatmL

08206.0

Example 2How many moles of hydrogen would be contained in 6.0 L of the gas at 101.4 kPa and 64oC?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Guided Practice #1What is the temperature of 0.456 mol of gas at 1 atm if the gas is held in a 10.0 L container?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Guided Practice #2What volume is occupied by 1.23 moles of methane, CH4, at 27oC and 1.59 atm?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Its time to see if you truly understand the Ideal Gas Law. ..

Closing What variables are needed to use the

Ideal Gas Law equation?

Warm Up: 3 Minutes

The pressure for an ideal gas is 72.8 kPa. If there are 4.6 moles in a 10.7 L container, calculate the temperature of the gas.

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Agenda

Warm Up: 7 Minutes Ideal Gas Law Video: 15 Minutes Guided Practice: 13 Minutes Independent Practice: 15 Minutes Closing: 3 Minutes

Announcements

Gas Law Quiz FRIDAY (Boyles, Charles, G. Lussac’s, Combined, Ideal)

Gas Law Exam 5/7

Today you will need:

Calculator Periodic Table

Ideal Gas Law-Part 2 Video1. Go to shschem.weebly.com (our class

Example 1What is the volume of 22.0 g carbon dioxide (CO2) at 312 K and 795 mmHg?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Uh oh…

We are given grams…but “n” needs to be in moles.

How do we go from grams to moles?

Use Molar Mass!

Review of Molar Mass

Example 1What is the volume of 22.0 g carbon dioxide (CO2) at 312 K and 795 mmHg?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Example 2How many grams of hydrogen gas (H2) would be contained in 5.35 L of the gas at 119.7 kPa and -29oC?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Guided Practice #1What is the temperature of 71.8 g nitrogen gas (N2) at 1 atm if the gas is held in a 10.0 L container?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Guided Practice #2What volume is occupied by 7.02 moles of sulfur dioxide, SO2, at 361oC and 14.07 atm?

KmolkPaL

KmolmmHgL

KmolatmL

08206.0

Its time to see if you truly understand the Ideal Gas Law. ..

Closing How does the ideal gas law relate P, V,

n, and T?

Warm Up: 4 Minutes

An ideal gas is trapped in a closed container. The pressure inside the container is 634 mmHg. If there are 38 g H2 at 98 ºC, calculate the volume of the container.

Agenda

Warm Up: 7 Minutes Gas Law Stoichiometry Video: 15 Minutes Guided Practice: 13 Minutes Independent Practice: 15 Minutes Closing: 3 Minutes

Gas Law Stoichiometry Video1. Go to shschem.weebly.com (our class

3. Watch video for May 14. Take notes on your handout

Remember this?

It’s time to do…

Gas Law Stoichiometry

Example 1The reaction of zinc and hydrochloric acid is shown below:

Zn + 2 HCl ZnCl2 + H2

If 17L of hydrogen gas are formed at a pressure of 2.6 atm and a temperature of 180 ºC, how many moles of zinc reacted?

Example 2How many grams of Mercury (II) Chloride will react with 0.567 L ammonia at 27.0 ºC and 115 kPa?

HgCl2 + 2 NH3 NH4Cl + Hg(NH2)Cl

Guided Practice #1The combustion of octane is shown below:

2 C8H18 + 25 O2 16 CO2 + 18 H2O

If 38L of carbon dioxide are formed at a pressure of 186 mmHg and a temperature of 146 K, how many moles of octane reacted?

Guided Practice #2How many grams of sodium hydrogen carbonate (NaHCO3) are needed to react to form 11.64 liters of carbon dioxide?

HNO3 + NaHCO3 NaNO3 + CO2 + H2O

Its time to see if you truly understand Gas Law

Stoichiometry. ..

Closing How does the ideal gas law relate P, V,

n, and T?

Warm Up: 5 Minutes

Zinc metal reacts with hydrochloric acid according to the reaction below:

Zn + 2 HCl 2 ZnCl2 + H2

If 14.5 L hydrogen gas were produced at a pressure of 4.7 atm and a temperature of 45 ºC, calculate the number of moles of hydrochloric acid that reacted. [Use R = 0.08206]

Agenda

Warm Up: 9 Minutes Quiz Expectations: 4 Minutes Gas Laws Quiz: 30 Minutes Closing: 2 Minutes

Material Covered

Boyle’s Law Charles Law G. Lussac’s Law Combined Gas Law Ideal Gas Law Gas Law Stoichiometry (Extra Credit)

To demonstrate mastery, we are shooting for

Check Point

What is your goal for this quiz?

Expectations for Quiz

Clear your desk of everything except a....

1. Pencil/Pen2. Calculator

All backpacks and binders on the floor

Expectations Students will keep eyes on own paper

Cheating will result in an automatic ZERO

Students will remain SILENT for the duration of the quiz

Good Luck!!

Quiz Correction:

For the Extra Credit problem:

Assume P = 1 atm and T = 0 ºC

Closing

How was your Quiz Today?

What topics do you feel you still need review on?

week 33 chemistry

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