when sulfur is burned in the presence of oxygen, sulfur trioxide is produced. if 3.4 x 10^24 atoms of sulfur react, how many liters of sulfur trioxide are produced?
S (s) + O2 (g) --> SO2(g)
2SO2 (g) + O2 (g) <--> 2 SO3 (g)
now using appropriate mol ratios you can solve...
3.4 x 10^24 S atoms (1 mol S/avagadros #)(2 mol SO3/1 mol S)
then you can use the mols of SO3 to solve for g (using molecular mass) and then litres...
To determine the number of liters of sulfur trioxide produced, we need to use the given amount of sulfur atoms to calculate the number of moles, and then use the molar ratio between sulfur and sulfur trioxide to convert the moles of sulfur trioxide, and finally, use the Ideal Gas Law to convert the moles of sulfur trioxide to liters.
Step 1: Convert sulfur atoms to moles of sulfur
We are given 3.4 x 10^24 atoms of sulfur. To convert this into moles, we need to divide the given number by Avogadro's number, which is 6.022 x 10^23 atoms/mol.
Number of moles of sulfur = (3.4 x 10^24 atoms) / (6.022 x 10^23 atoms/mol)
Step 2: Determine the molar ratio between sulfur and sulfur trioxide
The balanced chemical equation for the reaction is:
Sulfur + Oxygen → Sulfur Trioxide
From the equation, we can see that for every 1 mole of sulfur reacted, 1 mole of sulfur trioxide is produced. Therefore, the molar ratio between sulfur and sulfur trioxide is 1:1.
Step 3: Convert moles of sulfur trioxide to liters
To convert the moles of sulfur trioxide to liters, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P is the pressure (which isn't mentioned, so we will assume it to be standard pressure, 1 atm)
V is the volume in liters (the value we want to find)
n is the number of moles of sulfur trioxide
R is the ideal gas constant (0.08206 L·atm/(mol·K))
T is the temperature (which is not given, so we will also assume standard temperature, 273 K)
Rearranging the Ideal Gas Law equation to solve for V:
V = (nRT) / P
Substituting the values into the equation, we get:
V = (moles of sulfur trioxide) * (0.08206 L·atm/(mol·K)) * (273 K) / (1 atm)
Now, we can substitute the number of moles of sulfur trioxide from step 1 into the equation and calculate the final value to find the volume of sulfur trioxide produced in liters.