Consider the reaction CH4+ 2Cl2=CCl4. If .33 moles of CH4 is reacted with 1 mole of Cl2, how much CCl4 is produced?
What does the mole ratio here of 2:1 actually mean?
To find out how much CCl4 is produced, we need to determine the limiting reactant. The limiting reactant is the one that will be completely consumed and determines the amount of product that can be formed.
First, we need to calculate the number of moles of Cl2 available using the given information:
Number of moles of Cl2 = 1 mole
Next, we need to compare the moles of CH4 with the moles of Cl2 to determine which is limiting. Since the balanced equation states that it requires 2 moles of Cl2 for every 1 mole of CH4:
Moles of CH4 required = 2 × Number of moles of Cl2
Moles of CH4 required = 2 × 1 mole
Moles of CH4 required = 2 moles
Since we only have 0.33 moles of CH4, which is less than the required 2 moles, CH4 is the limiting reactant.
Now, we can calculate the moles of CCl4 produced using the stoichiometry of the balanced equation:
Moles of CCl4 produced = Number of moles of CH4 × (1 mole of CCl4 / 1 mole of CH4)
Moles of CCl4 produced = 0.33 moles × (1 mole of CCl4 / 1 mole of CH4)
Moles of CCl4 produced = 0.33 moles
Therefore, when reacting 0.33 moles of CH4 with 1 mole of Cl2, the amount of CCl4 produced is 0.33 moles.