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Chapter 11 Chemistry
| Question | Answer |
|---|---|
| your ears pop on a plane because... | the air pressure is higher in the air |
| if a container has a high # of particles, it will have... | high # of collisions & high pressure |
| if the temperature of a container is high, it will have... | high speed of particles, high # of collisions, high pressure |
| if a container is expanded, it will have... | high volume, low # of collisions, low pressure |
| a skate is more likely to break through ice than a shoe because... | it is the same force on a smaller area, increasing pressure |
| the pressure units of STP are... | 1 atm - 101.3kPa - 760 torr - 760 mmHg |
| in a manometer, the side with less pressure will... | be higher |
| in a manometer, the difference in the height of the columns is equal to... | the difference between the two pressures |
| the equation to calculate the pressure of gas in a manometer is... | P(gas) = P (atm) ± P (Hg) |
| if the air is higher on the open side of a manometer, the equation would include... | adding |
| the steps to solving a manometer equation are... | 1) convert pressure to correct units -- 2) decide to add or subtract -- 3) plug in and solve -- 4) round to at least two dp |
| dalton's law of partial pressure | total pressure = sum of partial pressure of each gas |
| dalton's law of partial pressure equation | P (total) = P1+P2+... |
| mole fraction equations | X1 = n1/n(total) ﹌ n (total) = n1+n2+... |
| partial pressure equations | X1 = P1/P(total) ﹌ P1 = X1 x P (total) |
| partial pressure SHORTCUT equation | P1 = n1/n(total) x P (total) |
| X1 stands for... | mole fraction |
| P1, P2, etc. stands for... | partial pressure |
| P (total) stands for... | total pressure |
| n1 stands for... | number of moles in gas #1 |
| n (total) stands for... | total number of moles |
| to find what percent a mole fraction is equal to, use the equation... | X1 x 100 = % |
| pressure and volume have a/an... | inverse relationship |
| temperature and pressure have a/an... | direct relationship |
| volume and temperature have a/an... | direct relationship |
| Boyle's Law | at a constant temp, the volume of a gas is inversely related to the pressure |
| Boyle's Equation | P1V1=P2V2 |
| Charles' Law | at constant pressure, the volume is directly related to the ABSOLUTE temp |
| Charles' Equation | V1/T1 = V2/T2 |
| Gay-Lussac Law | at constant volume, the pressure is directly related to the ABSOLUTE temp |
| Gay-Lussac Equation | P1/T1 = P2/T2 |
| Combined Gas Equation | P1V1/T1 = P2V2/T2 |
| when solving any gas law equations, make sure... | all variable have the same units & all temps are in kelvin |
| Celsius To Kelvin Equation | C°+273=K |
| a beaker must be fully filled with water before collecting gas because... | it minimizes reactions & makes the gas relatively pure |
| the water level will go down when a gas generator is in use because... | the gas generator exerts pressure |
| when using water to collect gas, it will never be completely pure because... | water will evaporate and become present |
| Collecting Gas Over Water Equation | P (total) = P (H2O) + P (dry gas) |
| at 25°C, water's pressure is... | 3.17kPa |
| Avogadro's Law | equal volumes of gases at the same temperature & pressure contain the same amount of molecules |
| Molar Volume | volume occupied by one mole of gas |
| at STP, 1 mol of a substance is equal to... | 22.4 L |
| the number of molecules in one mole is... | 6.022 x 10^23 |
| Gay-Lussac's Law Of Combining Volumes | at constant temperature & pressure, the volumes of gaseous reactants & products can be expressed at ratios of small whole numbers |
| the constant value for 'R' is... | 0.0821 |
| Density Equation | D=MP/RT |
| Units For PV=nRT | pressure in atm / volume in L / moles in moles / temperature in K / R in Latm/moleK |
| when given the grams in a PV=nRt problem... | convert to moles using stoich |
| Unit For Density | g/L |
| Unit For Molar Mass | g/mole |
| gases are nearly ideal with... | high temperature & low pressure |
| gases deviate from being ideal with... | high polarity & IMFA |
| ideal gases have... | no volume & no IMFA |
| Diffusion | random scattering of gas particles |
| Effusion | gas particles escape through a hole |
| Graham's Law Equation | r1/r2 = √m2/m1 |
| you decide to multiply or divide in Graham's Law by... | high mass, slower, multiply // low mass, faster, divide |
| Solving Graham's Law | 1: calculate molar mass // 2: write equation // 3: plug in & solve // 4: write the rate expression: (r gas 1 = # r gas 2) |
| Steps To Find Unknown Molar Mass | 1: write the rate statement (r gas 1 = # r gas 2) // rearrange the rate expressions |
Created by:
abievans
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