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Liters to<br />
Liters<br />
Define-<br />
Going from liters<br />
of one molecular<br />
compound to<br />
another<br />
Balance the equation.<br />
Write conversions (1<br />
mole of gas=22.4liters,<br />
mole to mole)<br />
Convert from the given<br />
units to the desired<br />
units in a conversion<br />
chart<br />
Limiting<br />
reagents<br />
The element that<br />
will run out first,<br />
the smallest<br />
amount.<br />
Write conversions, Set<br />
up two equations to the<br />
same units. The smallest<br />
is the limiting reagent<br />
For the balanced equation<br />
shown below, what would be<br />
the limiting reagent if 83.2<br />
grams of Al were reacted<br />
with 584 grams of MnO?<br />
2Al+3MnO=>Al2O3+3Mn<br />
For the balanced<br />
equation shown below,<br />
what would be the<br />
limiting reagent if 91.0<br />
grams of CO were<br />
reacted with 19.8 grams<br />
of H2?<br />
3CO+7H2=>C3H8+3H2O<br />
Percent<br />
yield<br />
Define<br />
Percent yield is the<br />
percent ratio of<br />
actual yield to the<br />
theoretical yield<br />
Steps<br />
Balance your equation.<br />
calculate the molar<br />
mass of the element of<br />
compound given and<br />
the one you’re finding.<br />
Write conversions.<br />
Using the conversion<br />
table convert from the<br />
element or molecular<br />
compound given to the<br />
compound you are<br />
looking for. The answer<br />
is your theoretical yield.<br />
Take the theoretical<br />
yield and multiply it by<br />
the percent yield<br />
(decimal form) to find<br />
the actual yield.<br />
For the balanced equation<br />
shown below, if the reaction<br />
of 62.0 grams of H2<br />
produces<br />
a 81.5% yield, how many<br />
grams of H2O would be<br />
produced ?<br />
For the balanced<br />
equation shown below, if<br />
the reaction of 90.1<br />
grams of O2<br />
produces a<br />
76.5% yield, how many<br />
grams of H2O would be<br />
produced ?<br />
117
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