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| What uniformly fill any container, are easily compressed, and mix completely with like substances? |
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| Earth's atmosphere is about what percent of nitrogen? |
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| Earth's atmosphere is about what percentage of oxygen gas? |
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| The universes about what percent of hydrogen gas? |
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| What results from the weight of the air (mass of air is being pulled toward the center of earth by gravity)? |
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| Who invented the barometer in 1643? |
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| device used to measure atmospheric pressure |
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Definition
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| What corresponds to bad weather? |
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Definition
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| What is atmospheric pressure at sea level? |
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Definition
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| What is the atmospheric pressure in higher elevations (such as Breckenridge, Colorado)? |
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| what is measured in Newtons? |
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Definition
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| What is is measured in square meters? |
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Definition
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| What is the Pascal the SI unit for? |
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Definition
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Term
| How many Pascals are in one atmosphere? |
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| How many inches of Hg are in one atm? |
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Definition
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| How many pounds per square inch are in one atm? |
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Definition
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Term
| What are gases that obey the gas laws termed? |
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Definition
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Term
| What make gases deviate from ideal gas behavior? |
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Definition
| high pressure and low temperature (makes them closer together) |
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Term
| Who was the first to fill a balloon with hydrogen gas and first to make a solo balloon flight? |
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| The volumes of all gases extrapolate to what? |
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Definition
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| What is the ideal gas law? |
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Definition
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Term
| What is the molar volume of one mole of a gas at STP? |
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Definition
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Term
| What is the molar mass formula? |
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Definition
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Term
| for a mixture of gases in a container, the total pressure exerted is the sum of the pressures that each gas in a mixture of gases in a container depends on the number of moles of that gas |
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Definition
| Dalton's Law of Partial Pressure |
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Term
| What is made from sodium azide? |
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Definition
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| balance the decomposition of sodium azide |
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Definition
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Definition
| summarize observed behavior |
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Definition
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| When are models considered successful? |
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Definition
| if i explains the observed behavior in question and predicts correctly the result of future experiments |
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Term
| Why is the volume of an individual particle assumed to be zero? |
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Definition
| particles are so small compared with distances between them |
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Term
| What are the causes of pressure exerted by the gas? |
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Definition
| particles are in constant motion so collisions of the particles with walls are the causes |
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Term
| particles are assumed to exert nor forces on each other |
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Definition
| they are assumed neither to attract nor repel each other |
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Term
| What is assumed to be directly proportional to the Kelvin temp of the gas (ideal not real) |
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Definition
| average kinetic energy of a collection of gas particles |
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Term
| What is the root mean square velocity formula? |
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Definition
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Term
| What are the units for root mean square velocity? |
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Definition
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Term
| What is the value for R in the root mean square velocity formula? |
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Definition
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Term
| What is the si unit for energy |
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Definition
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Term
| What is the average distance a particle travels between collisions in a particular gas sample |
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Definition
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Term
| What is the ration of the number of moles of a given component in a mixture both total number of moles in the mixture? |
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Definition
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Definition
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Term
| passage of a gash through a tiny orifice into a vacuum |
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Definition
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Term
| rate of the mixing of gases |
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Definition
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Term
| measure the speed at which the gas is transferred into the chamber |
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Definition
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Term
| What is the formula for Graham's law of effusion? |
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Definition
Rate of effusion for gas 1/rate of effusion for gas 2
square root of M2/ square root of M1 |
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Term
| Who developed an equation for real gases? |
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Definition
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Term
| layer of atmosphere closest to earth with all clouds and weather |
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Definition
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Term
| What are the two main sources of pollution? |
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Definition
| transportation and production of electricity |
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Term
| Would gases act more ideally with a few moles involved or a great number of moles involved? |
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Definition
| few, gases don't like to be close together |
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Term
| One mole of gas contains how many molecules? |
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Definition
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Term
| One mole of any gas occupies how many liters at STP? |
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Definition
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Term
| Diatomic molecules exhibit what kind of bonding? (share electrons equally) |
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Definition
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Term
| Which of the following gases diffuse faster? Oxygen gas or Butane gas? Why? |
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Definition
| Oxygen, mass of oxygen is less than mass of butane |
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Term
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Definition
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Term
| If all the gases have the same temperature, what happens? |
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Definition
| they all have the same kinetic energy |
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Term
| If volume increases on a gas, what happens to pressure? |
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Definition
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Term
| Gases act most ideally under what conditions? |
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Definition
| high temperature and low pressure |
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Term
| What factor is used to determine if gases have the same partial pressures? |
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Definition
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Term
| Would a gas exert greater pressure as an ideal gas or as a real gas? |
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