Given the following reaction:
\qquad
R1_RATIO === 1 ? "" : R1_RATIOR1 +
R2_RATIO === 1 ? "" : R2_RATIOR2 \rightarrow
P1_RATIO === 1 ? "" : P1_RATIOP1
+ P2_RATIO === 1 ? "" : P2_RATIOP2
How many grams of P1 will be produced from
R1_MASS \text{g} of R1 and
R2_MASS \text{g} of R2?
\dfrac{R1_MASS \cancel{\text{g}}}{R1_MOLAR_MASS \cancel{\text{g}} / \text{mol}} =
\blue{\text{ R1_MOL plural_form(MOLE, R1_MOL)}} \text{ OF }R1
[Explain]
First we want to convert the given amount of R1 from grams to moles. To do this, we divide
the given amount of R1 by the molar mass of R1.
\dfrac{\text{GRAMS_OF }R1}{\text{MOLAR_MASS_OF }R1} = \text{MOLES_OF }R1
To find the molar mass of R1, we look up the atomic weight of each atom in a molecule of
R1 in the periodic table and add them together.
In this case, it's R1_MOLAR_MASS \text{g/mol}.
Dividing the given R1_MASS \text{g} of R1 by the molar mass of
R1_MOLAR_MASS \text{g/mol} tells us we're starting with
R1_MOL\text{ plural_form(MOLE, R1_MOL) OF }R1.
\dfrac{R2_MASS \cancel{\text{g}}}{R2_MOLAR_MASS \cancel{\text{g}} / \text{mol}} =
\green{\text{ plural(R2_MOL, "mole")}} \text{ OF }R2
[Explain]
We want to convert the given amount of R2 from grams to moles. To do this, we divide
the given amount of R2 by the molar mass of R2.
\dfrac{\text{GRAMS_OF }R2}{\text{MOLAR_MASS_OF }R2} = \text{MOLES_OF }R2
To find the molar mass of R2, we look up the atomic weight of each atom in a molecule of
R2 in the periodic table and add them together.
In this case, it's R2_MOLAR_MASS \text{g/mol}.
Dividing the given R2_MASS \text{g} of R2 by the molar mass of
R2_MOLAR_MASS \text{g/mol} tells us we're starting with
\text{ R2_MOL plural_form(MOLE, R2_MOL)} \text{ OF }R2.
The mole ratio of \dfrac{R1}{R2} in the reaction is
\dfrac{R1_RATIO}{R2_RATIO}.
[Explain]
The reaction is \blue{R1_RATIO}R1 +
\red{R2_RATIO}R2 \rightarrow
P1_RATIOP1 + P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(R2_RATIO) R2 molecule
The reaction is \blue{R1_RATIO}R1 +
\red{R2_RATIO}R2 \rightarrow
P1_RATIOP1 + P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(R2_RATIO) R2 molecules
\qquad
\dfrac{R1}{R2} = \dfrac{R1_RATIO}{R2_RATIO} =
\dfrac{\blue{\text{ R1_MOL plural_form(MOLE, R1_MOL)}}}{x}
[Show alternate approach]
\dfrac{R1}{R2} = \dfrac{R1_RATIO}{R2_RATIO} =
\dfrac{x}{\green{\text{ plural(R2_MOL, "mole")}}}
Instead of finding out how much R2 we need to react with all of our R1, we could
figure out how much R1 we need to react with all of our R2. In this case,
x = \text{ roundTo(3, R2_MOL * R1_RATIO / R2_RATIO) plural_form(MOLE, roundTo(3, R2_MOL * R1_RATIO / R2_RATIO))} of
R1 needed, which
is more than we have. Therefore R1 is the limiting reagent.
x = \text{ roundTo(3, R1_MOL * R2_RATIO / R1_RATIO) plural_form(MOLE, roundTo(3, R1_MOL * R2_RATIO / R1_RATIO))} of
R2 needed.
We have \text{ R2_MOL plural_form(MOLE, R2_MOL)} of R2, which is more
than we need. Therefore R1 is the limiting reagent.
The mole ratio of \dfrac{R1}{P1} in the reaction is
\dfrac{R1_RATIO}{P1_RATIO}.
[Explain]
The reaction is \blue{R1_RATIO}R1 +
R2_RATIOR2 \rightarrow
\red{P1_RATIO}P1
+ P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(P1_RATIO) P1 molecule.
The reaction is \blue{R1_RATIO}R1 +
R2_RATIOR2 \rightarrow
\red{P1_RATIO}P1
+ P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(P1_RATIO) P1 molecules.
\qquad
\dfrac{R1}{P1} = \dfrac{R1_RATIO}{P1_RATIO} =
\dfrac{\blue{\text{ R1_MOL plural_form(MOLE, R1_MOL)}}}{x}
x = \text{ P1_MOL plural_form(MOLE, P1_MOL)} of P1 produced.
The mole ratio of \dfrac{R1}{R2} in the reaction is
\dfrac{R1_RATIO}{R2_RATIO}.
[Explain]
The reaction is \blue{R1_RATIO}R1 +
\red{R2_RATIO}R2 \rightarrow
P1_RATIOP1 + P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(R2_RATIO) R2 molecule.
The reaction is \blue{R1_RATIO}R1 +
\red{R2_RATIO}R2 \rightarrow
P1_RATIOP1 + P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R1_RATIO) R1 for every
cardinalThrough20(R2_RATIO) R2 molecules.
\qquad
\dfrac{R1}{R2} = \dfrac{R1_RATIO}{R2_RATIO} =
\dfrac{x}{\green{\text{ R2_MOL plural_form(MOLE, R2_MOL)}}}
\qquad
[Show alternate approach]
\dfrac{R1}{R2} = \dfrac{R1_RATIO}{R2_RATIO} =
\dfrac{\blue{\text{ R1_MOL plural_form(MOLE, R1_MOL)}}}{x}
Instead of finding out how much R1 we need to react with all of our R2, we could
figure out how much R2 we need to react with all of our R1. In this case,
x = \text{ roundTo(3, R1_MOL * R2_RATIO / R1_RATIO) plural_form(MOLE, roundTo(3, R1_MOL * R2_RATIO / R1_RATIO))} of
R2 needed, which
is more than we have. Therefore R2 is the limiting reagent.
x = \text{ roundTo(3, R2_MOL * R1_RATIO / R2_RATIO) plural_form(MOLE, roundTo(3, R2_MOL * R1_RATIO / R2_RATIO))} of
R1 needed.
We have \text{ R1_MOL plural_form(MOLE, R1_MOL)} of R1, which is more
than we need. Therefore R2 is the limiting reagent.
The mole ratio of \dfrac{R2}{P1} in the reaction is
\dfrac{R2_RATIO}{P1_RATIO}.
[Explain]
The reaction is R1_RATIOR1 +
\blue{R2_RATIO}R2 \rightarrow
\red{P1_RATIO}P1
+ P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R2_RATIO) R2 for every
cardinalThrough20(P1_RATIO) P1 molecule.
The reaction is R1_RATIOR1 +
\blue{R2_RATIO}R2 \rightarrow
\red{P1_RATIO}P1
+ P2_RATIOP2.
The coefficients in front of each molecule tell us in what ratios the molecules react. In this case
cardinalThrough20(R2_RATIO) R2 for every
cardinalThrough20(P1_RATIO) P1 molecules.
\qquad
\dfrac{R2}{P1} = \dfrac{R2_RATIO}{P1_RATIO} =
\dfrac{\green{\text{ R2_MOL plural_form(MOLE, R2_MOL)}}}{x}
x = \text{ P1_MOL plural_form(MOLE, P1_MOL)} of P1 produced.
\cancel{\text{P1_MOL plural_form(MOLE, P1_MOL)}}
P1 \times \dfrac{P1_MOLAR_MASS \text{g}}{\cancel{\text{plural_form(MOLE, 1)}}} =
\text{ P1_MASS plural_form(GRAM, P1_MASS)} \text{ OF }P1