what volume of oxygen is needed to react with solid sulfur to form 6.20 L of sulfur dioxide according to the reaction S(s) + O2(g) yield SO2(g)
At STP?
S + O2 ==> SO2
mols SO2 = 6.20/22.4 = ?
mols O2 = the same
? mols SO2 x (22.4 L/1 mol) = 6.20 L O2 needed.
To determine the volume of oxygen needed to react with solid sulfur, we need to use the balanced chemical equation and the ideal gas law.
The balanced chemical equation between sulfur (S), oxygen gas (O2), and sulfur dioxide (SO2) is:
S(s) + O2(g) → SO2(g)
According to the equation, we know that one mole of sulfur reacts with one mole of oxygen to form one mole of sulfur dioxide.
Given that the desired volume of sulfur dioxide is 6.20 L, we need to convert this volume into the number of moles using the ideal gas law, which states that:
PV = nRT
Where:
P is the pressure of the gas,
V is the volume of the gas,
n is the number of moles of the gas,
R is the ideal gas constant (0.0821 L·atm/(K·mol)),
T is the temperature in Kelvin.
Let's assume that the pressure and temperature are constant, so the ideal gas law simplifies to:
V = nR / P
Now, we can calculate the number of moles of sulfur dioxide using the ideal gas law equation:
n = PV / RT
Assuming the pressure and temperature are known, substitute the values into the equation to find the number of moles.
Finally, since one mole of sulfur reacts with one mole of oxygen, the volume of oxygen that reacts can be determined.
To determine the volume of oxygen needed to react with solid sulfur, we need to use the balanced chemical equation for the reaction:
S(s) + O2(g) → SO2(g)
The coefficients in the balanced equation indicate the mole ratio between sulfur, oxygen, and sulfur dioxide. Since the equation is balanced as 1:1:1, it means that one mole of sulfur reacts with one mole of oxygen to produce one mole of sulfur dioxide.
1. Convert the given volume of sulfur dioxide (SO2) to moles using the ideal gas law equation: PV = nRT.
To do this, we need to know the temperature (T) and pressure (P) at which the sulfur dioxide is measured. Let's assume standard temperature and pressure (STP), which is 0 °C (273 K) and 1 atmosphere (1 atm), respectively.
Using the ideal gas law equation, which is PV = nRT, we rearrange the equation to solve for moles (n):
n = PV / RT
Since STP conditions are given, the gas constant R is equal to 0.0821 L·atm/(mol·K).
Let's assume the pressure (P) of sulfur dioxide is 1 atm. Therefore:
n = (6.20 L)(1 atm) / (0.0821 L·atm/(mol·K))(273 K)
Calculate the value of n using the above equation.
2. Determine the volume of oxygen (O2) needed based on the mole ratio from the balanced equation.
Since the balanced equation is 1:1, it means that one mole of oxygen reacts with one mole of sulfur dioxide. Therefore, the molar volume of oxygen required is the same as moles of sulfur dioxide calculated in step 1.
3. Convert the moles of oxygen to volume using the ideal gas law equation.
Using the ideal gas law equation, PV = nRT, and rearranging the equation to solve for volume (V):
V = nRT / P
Assume the temperature and pressure are the same as given in step 1, which is 0 °C (273 K) and 1 atm, respectively.
Substitute the value of n (calculated in step 1) into the equation and solve for volume (V).
The result will be the volume of oxygen required to react with solid sulfur and produce 6.20 L of sulfur dioxide.