Identify the limiting reagent and the volume of product formed with 11L CS2 reacts with 18L O2 to prduce CO2 gas and SO2 gas.
CS2+3O2-->CO2+2SO2
i don't get it
11 L CS2 needs 33 L O2 and you have only 18 L O2. So which is the limiting reagent? oxygen or CS2?
To identify the limiting reagent and calculate the volume of product formed, we will follow these steps:
Step 1: Convert the given volumes of CS2 and O2 to moles.
To do this, we need to know the molar volume of each gas at the given conditions. Let's assume the molar volume for both CS2 and O2 is 22.4 L/mol (which is the molar volume at standard temperature and pressure, STP). This assumption allows us to convert volume to moles.
Moles of CS2 = Volume of CS2 / Molar volume of CS2
Moles of CS2 = 11 L / 22.4 L/mol
Moles of O2 = Volume of O2 / Molar volume of O2
Moles of O2 = 18 L / 22.4 L/mol
Step 2: Determine the stoichiometric ratio between CS2 and O2 based on the balanced chemical equation.
From the balanced equation: CS2 + 3O2 → CO2 + 2SO2, we can see that the ratio of CS2 to O2 is 1:3.
Step 3: Compare the moles of CS2 and O2 to find the limiting reagent.
To find the limiting reagent, we need to determine which reactant is in excess and which is limiting. We compare the moles of the two reactants using the stoichiometric ratio determined in step 2.
Moles of CS2 = 11 L / 22.4 L/mol = 0.491 moles (approx.)
Moles of O2 = 18 L / 22.4 L/mol = 0.804 moles (approx.)
Since the stoichiometric ratio of CS2 to O2 is 1:3, it means that for every 1 mole of CS2, we need 3 moles of O2. In this case, we have less moles of CS2 (0.491 moles) compared to O2 (0.804 moles). Therefore, CS2 is the limiting reagent.
Step 4: Calculate the moles of product formed.
To calculate the moles of product formed, we need to use the stoichiometric ratio of the balanced equation.
From the balanced equation: CS2 + 3O2 → CO2 + 2SO2, we know that for every mole of CS2, we produce 1 mole of CO2 and 2 moles of SO2.
Since CS2 is the limiting reagent, the moles of CO2 and SO2 formed will be equal to the moles of CS2.
Moles of CO2 = 0.491 moles (approx.)
Moles of SO2 = 2 * Moles of CS2 = 2 * 0.491 moles = 0.982 moles (approx.)
Step 5: Convert the moles of CO2 and SO2 to volume using the molar volume at STP.
To convert the moles of the products to volume, we'll use the molar volume of gases at STP.
Volume of CO2 = Moles of CO2 * Molar volume of CO2
Volume of CO2 = 0.491 moles * 22.4 L/mol
Volume of SO2 = Moles of SO2 * Molar volume of SO2
Volume of SO2 = 0.982 moles * 22.4 L/mol
Step 6: Calculate the volume of product formed.
Using the values from step 5, calculate the volume of the product formed.
Volume of CO2 = 0.491 moles * 22.4 L/mol = 11.0 L
Volume of SO2 = 0.982 moles * 22.4 L/mol = 22.0 L
Therefore, the volume of CO2 formed is 11.0 L, and the volume of SO2 formed is 22.0 L.
When you have gases at the same temperature and pressure, the volume ratio is equal to the mole ratio. The ratio of the coefficients in the chemical equation can be used as mole ratios OR volume ratios:
(11L CS2)(3 L O2 / 1 L CS2) = 33 L O2 *needed*
Since only 18 L O2 are *available*, which is the limiting reagent?