Given that 14.2 liters of chlorine gas react according to the following equation...
Cl2 + 3 F2---> 2ClF3
Question: If all gases were under the same conditions of temperature and pressure,what volume of chlorine triflouride would be produced? (using mole ratio)
If all reactants and products are gases, then L may be treated as moles.
14.2L Cl2 x (2 moles ClF3/1 mole Cl2) =
14.2 L x (2/1) = ?? L ClF3.
To find the volume of chlorine trifluoride produced, we need to use the mole ratio from the balanced equation. The mole ratio tells us how many moles of one substance react with another. In this case, the mole ratio is 2 moles of ClF3 to 1 mole of Cl2.
To solve the problem, we'll follow these steps:
Step 1: Convert the given volume of chlorine gas (Cl2) to moles.
Given: Volume of Cl2 = 14.2 liters
To convert liters to moles, we need to use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Since the problem states that all gases are under the same conditions of temperature and pressure, we can assume the pressure and temperature are constant. Therefore, we only need to convert the given volume to moles.
To convert liters to moles, we'll use the following formula:
moles = volume (in liters) / molar volume at STP
The molar volume at STP (Standard Temperature and Pressure) is approximately 22.4 liters/mol.
moles of Cl2 = 14.2 liters / 22.4 liters/mol
Step 2: Use the mole ratio from the balanced equation to determine moles of chlorine trifluoride (ClF3) produced.
Mole ratio: 2 mol ClF3 / 1 mol Cl2
moles of ClF3 = moles of Cl2 * (2 mol ClF3 / 1 mol Cl2)
Step 3: Convert moles of chlorine trifluoride to volume.
To convert moles to volume, we'll use the molar volume at STP again.
volume of ClF3 = moles of ClF3 * molar volume at STP
Remember to keep the units consistent throughout the calculations.
By following these steps, you can determine the volume of chlorine trifluoride produced using the given mole ratio and the volume of chlorine gas.