REV CH11 bold means show work NAME_______________________
1. Gay-Lussac said gases react in what kind of ratios?
2. Avogadro said equal volumes of gases (at the same conditions) contain what?
3. Standard molar volume is what at what? Give numbers for STP
4. Solve the ideal gas equation for R. What does R represent? solve igl for V.
5. Coefficients in an equation always represent what, but can also represent what when all the reactants are what?
6. What is the difference between effusion and diffusion?
7. Which will diffuse/ effuse faster at the same temperature, hydrogen or oxygen gas? Why? This is an example of what law? Calculate how many times faster. (see p 388 of text) answer the same question for ammonia and carbon monoxide.
8. a. * 0.15mole of gas occupies 250mL and is at 5atm, what is the temp in degrees C?
b. What mass of butane would occupy 85mL at 90Kpa and 10 degrees C ?
c. 80 mL of butane collected at 763mmHg and 20degreesC would have what volume at 2atm and 100 degrees C?
Use this equation for for the following N2 + 3H2 = 2NH3
9. *If 12 L of hydrogen were used how many L of ammonia result?
10. If 14g of nitrogen are used, how many moles of hydrogen result?
11. *If 30g hydrogen are used how many L of ammonia result (at STP)?
Butane Lab (collected over water):
Data – mass of lighter before 25.48g; after 25.27g; temp 19C, pressure 754torr, vol 85mL
(hint: find pressure of dry butane)
1. find the moles of butane (C4H10) using IGL
2. find moles of butane using mass and molar mass
3. list some properties of butane
4. define volatile; give an example of something volatile & something nonvolatile
5. how can graduated cylinders be kept from breaking?
6. explain why butane is liquid inside, but gas outside the lighter
7. describe the boiling pt and density of butane
Review lab calc and conclusions, then answer: *write the 2 equations for the reactions Include states
Acid –metal:
Combustion of hydrogen:
and then predict how many moles of hydrogen gas could be produced from 3 moles of zinc metal, if you had an excess of acid.
1. # molecules in 0.5mole carbon dioxide
2. volume of 15 moles of hydrogen gas at STP
3. volume of 120g of ammonia (NH3) at STP
1. volume of .0124moles of oxygen gas at 95Kpa and 50 degrees C
2. mass of 25L of carbon dioxide at 3atm and 20 degrees C
demonstrations:
list demonstrations from this chapter, and describe chemical principles illustrated in each.
instruments:
be able to read thermometer and barometer in correct units and convert those units to other units that we use.