# Gas Laws

### 35 terms by peoneill Teacher

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### decreases

When pressure increases, volume _____.

### increases

When temperature increases, pressure _____.

### increases

When temperature increases, volume _____.

mm Hg

atm

psi

Kelvin

Celsius

liter

milliliter

PV = nRT

P

V

n

R

T

### 1) Particles do not take up space. 2) Particles bounce off of each other without losing energy. 3) Particles are not attracted to one another. (no intermolecular forces)

3 Rules for ideal gases (vs real gases)

### Combined Gas Law

P₁V₁ / T₁ = P₂V₂ / T₂

### 1) Particles are small and inert. 2) Temperature is high. 3) Pressure is low.

3 Conditions when real gases act almost exactly like ideal gases.

### 1) Temperature must be in kelvins 2) Units for P1 must match P2 (and units for V1 must match V2)

2 Rules for units on the combined gas law (P₁V₁ / T₁ = P₂V₂ / T₂)

### Graham's Law

Rate₁/Rate₂ = sq rt(M₂)/sq rt (M₁)

### 1) The right side of the equation flips so that 2 is over 1. 2) Rate = amount/time

2 Rules for on Graham's Law
Rate₁/Rate₂ = sq rt(M₂)/sq rt (M₁)

### (all units must match the gas constant R) 1) Temperature must be in kelvins. 2) Pressure must be in atm. 3) Volume must be in L.

3 Rules for units on Ideal gas law
(PV = nRT)

### Mass can be used to find n (or conversely, n can be used to find mass) by converting between moles and grams.

Mass in the ideal gas law
(PV = nRT)

### effusion

the process that occurs when a gas escapes through a tiny hole in its container

### rate (described in terms of time)

= 1/time (inverse)

= amount

q = mc delta T

c

q

delta

m

Calorie (cal)

### specific heat (definition)

the heat required to raise the temperature of 1g of a substance 1°C

### specific heat of water

basis for the calorie

Example: