Term
| The 4 properties of a gas that can be measured are |
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Definition
| volume, pressure, temperature and number of particles (or moles) |
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Term
| How do you convert a Celsius temperature to a Kelvin temperature? |
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Definition
| Add 273 to the Celsius temperature. |
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Term
| What is room temperature in Celsius? |
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Definition
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Term
| Convert -50 °C to Kelvin. |
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Definition
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Term
| These two gases make up most of the troposphere (lowest level of the atmosphere) |
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Definition
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Term
| The 3 levels of the atomsphere are called the ____________, ______________ and ______________. |
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Definition
| Troposphere, Stratosphere, and Mesosphere |
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Term
| The levels of the atmosphere are defined by looking at changes in which property of the atmosphere? |
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Definition
| The temperature. It drops as you rise into the troposphere, then it rises again through the stratosphere, and finally it drops as you enter the mesosphere. |
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Term
As altitude increases, air pressure
(rises / drops / stays the same / fluctuates) |
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Definition
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Term
| What causes a temperature increase in the stratosphere? |
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Definition
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Term
| The device that measures air pressure is called a ____________ and it is filled with this liquid. |
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Definition
| barometer; filled with mercury (Hg). |
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Term
| As you increase altitude, the air gets "thinner". If air is "thinner" there are (more / fewer) molecules. |
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Definition
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Term
| Which creates a higher pressure on a desk surface - a book resting on its spine or a book lying flat, and why? |
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Definition
The book on its spine. Both situations have the same force acting on the desk (the weight of the book) but when the book is one its spine the force is acting over a smaller area, so the pressure is higher.
Pressure = force/area. |
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Term
| This scientist studied the relationship between gas volumes and temperatures. |
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Definition
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Term
| This scientist studied the relationship between gas volumes and pressures. |
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Definition
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Term
| This scientist studied the relationship between gas pressures and temperatures. |
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Definition
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Term
| The relationship between a gas' volume and its temperature is (direct / inverse). |
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Definition
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Term
| An inverse relationship exists between a gas' pressure and its (temperature / volume). |
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Definition
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Term
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Definition
Standard temperature and pressure.
0 °C and 1 atm
This doesn't mean "normal" temperature and pressure.
It just is a temperature and pressure that scientists use to report gas volumes at. |
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Term
| The equation for Gay-Lussac's law is |
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Definition
P1/T1 = P2/T2
Remember that temperature must be in Kelvin!
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Term
| The equation for Charles' Law is |
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Definition
V1/T1 = V2/T2
Remember that temperature must be in Kelvin!
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Term
| The equation for Boyle's Law is |
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Definition
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Term
| At STP, the volume occupied by one mole of any gas is |
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Definition
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Term
| In the reaction __ N2 + ___ H2 → ___ NH3, how many liters of ammonia are produced from 6 liters of H2? |
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Definition
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Term
| In the reaction __ N2 + ___ H2 → ___ NH3, how many moles of ammonia are produced from 84 grams of N2? |
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Definition
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Term
| A gas occupies a volume of 15 mL at 300 K. If the temperature rises to 500 K, what is the new volume of the gas? |
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Definition
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Term
| A gas at a temperature of 250 K exerts a pressure of 1.5 atm in a rigid box. If the temperature drops to 150 K, what is the new pressure of the gas? |
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Definition
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Term
| If the volume of a gas sample is 2 Liters when the pressure is normal atmospheric pressure, what will the new volume be if the pressure drops to 0.4 atm? |
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Definition
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Term
| In the reaction __ H2 + ___ O2 → ___ H2O, how many liters of water vapor are produced from 4 liters of O2? |
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Definition
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Term
| If all the reactants and products are gases in a chemical reaction, then the coefficients of a balanced equation can be interpreted as moles or ________. |
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Definition
| Liters (or any volume unit). |
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Term
| Imagine a gas sample in a rigid, fixed-volume container. If that container is heated, the gas sample will rise in temperature and its density will (increase / decrease / not change). |
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Definition
| not change! Density is mass/volume. By heating the gas, its pressure will rise, but you are not affecting the mass of the sample nor the volume it occupies, since it is in a rigid (fixed-volume) container. |
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