wake-up
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Wake-up. Write the formula for Charles Law. Write the formula for Boyle’s Law. Bromine gas has a pressure of 536.8 mmHg. When it is dispensed into a new container, its pressure becomes 784.6 mmHg with a new volume of 412.3 mL. What was the original volume? Identify the Law for #3. - PowerPoint PPT PresentationTRANSCRIPT
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Wake-up1. Write the formula for Charles Law.2. Write the formula for Boyle’s Law.3. Bromine gas has a pressure of 536.8 mmHg.
When it is dispensed into a new container, its pressure becomes 784.6 mmHg with a new volume of 412.3 mL. What was the original volume?
4. Identify the Law for #3.
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Ideal Gas Laws
What is the IDEAL GAS LAW?What are the variables involved?
What is Avogadro’s Law and didn’t I already learn about him with the mole?
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What is an Ideal Gas?
1. Made up of molecules which are in constant random motion in straight lines.
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What is an Ideal Gas?
2. The volume of the molecules is negligibly small compared to the volume occupied by the gas
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What is an Ideal Gas?
3. All collisions are perfectly elastic. (There is no loss of kinetic energy during the collision.)
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Ideal Gas Law EquationEquation is on the Reference Table
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What is R?
R is called the Ideal Gas Constant or Universal Gas Constant
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Gas Constant ValueSee Reference Table
0.0821 L atm
mole K
62.4
8.314 L kPa mole K
L mmHg mole K
What is the difference between each constant?
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Gas Constant ValueSee Reference Table
0.0821 L atm
mole K
62.4
8.314 L kPa mole K
L mmHg mole K
Units of Pressure – Select constant by units used in problem
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Proper units of Ideal Gas Formula
When using the Ideal Gas Formula, use correct units!!! Check units before use equation.
P = Pressure (atm)V = Volume (L)
n = Number of moles (mol)R = Gas constant L atm mol K
T = Temperature (K)
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Example #1How many moles of N2 are in a 750 mL vessel at
26 degrees Celsius and 625 mm Hg?P = 625 mmHg
V = 750mL 0.750 Ln = ?
R = 62.4 L mmHg mol KT = 26°C 299 K
(625)(0.75) = (n)(62.4)(299)468.75 = (18657.6)(n)
N = 0.025 mol
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Example #2If I have 17 moles of gas at a temperature of 67 0C, and a
volume of 88.89 liters, what is the pressure (kPa) of the gas?
P = ? kPaV = 88.89 Ln = 17 mol
R = 8.314 L kPa mol KT = 67°C 340 K
(P)(88.89) = (17)(8.314)(340)(P)(88.89) = (48054.92)
P = 540.6 kPa
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Example #3If I have 7.7 moles of gas at a pressure of 0.09 atm and at a temperature of 56 0C, what is the volume of the container
that the gas is in?
P = 0.09 atmV = ?
n = 7.7 molR = 0.0821 L atm mol KT = 56°C 329 K
(0.09)(V) = (7.7)(0.0821)(329)(0.09)(V) = (207.98)
N = 2310.9 L