A 2.5L flask contains 0.25mol each of so2 and n2 gas at 27 ° c. calculate the partial pressure exerted by each gas and also the total pressure exerted by each gas and the total pressure. name the law on which it is based
To calculate the partial pressure exerted by each gas and the total pressure, we can use Dalton's Law of Partial Pressures, which states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each gas.
Let's calculate the partial pressure exerted by each gas:
1. SO2 (Sulfur Dioxide):
- Number of moles (n) = 0.25 mol
- Volume (V) = 2.5 L
- Temperature (T) = 27 °C = 27 + 273 = 300 K
To find the partial pressure of SO2, we can use the Ideal Gas Law:
PV = nRT
Rearranging the formula to solve for pressure (P):
P = nRT / V
Plugging in the values:
P(SO2) = (0.25 mol × 0.0821 atm·L/mol·K × 300 K) / 2.5 L
P(SO2) = 0.0309 atm
2. N2 (Nitrogen):
- Number of moles (n) = 0.25 mol (same as SO2)
- Volume (V) = 2.5 L (same as SO2)
- Temperature (T) = 27 °C = 300 K (same as SO2)
Using the Ideal Gas Law:
P = nRT / V
Plugging in the values:
P(N2) = (0.25 mol × 0.0821 atm·L/mol·K × 300 K) / 2.5 L
P(N2) = 0.0309 atm
Therefore, the partial pressure exerted by each gas is 0.0309 atm for both SO2 and N2.
To calculate the total pressure exerted by the gases, we sum up the partial pressures:
Total Pressure = P(SO2) + P(N2)
Total Pressure = 0.0309 atm + 0.0309 atm
Total Pressure = 0.0618 atm
So, the total pressure exerted by the gases is 0.0618 atm.
The law on which these calculations are based is Dalton's Law of Partial Pressures.
To calculate the partial pressure exerted by each gas and the total pressure, we can use the ideal gas law equation. The ideal gas law is based on the principles of the ideal gas, which assumes that gas molecules have negligible volume and do not interact with each other.
The ideal gas law equation is represented as:
PV = nRT
Where:
P = Pressure (in Pascal or atm)
V = Volume (in liters)
n = Number of moles
R = Ideal gas constant (0.0821 L⋅atm/mol⋅K)
T = Temperature (in Kelvin)
First, we need to convert the temperature from degrees Celsius to Kelvin. The formula to convert Celsius to Kelvin is given by:
T(K) = T(°C) + 273.15
Given that the temperature is 27 °C, we can convert it to Kelvin:
T(K) = 27 + 273.15
T(K) = 300.15 K
Now, let's calculate the partial pressure of each gas:
Partial pressure of SO2 = (0.25 mol) * (0.0821 L⋅atm/mol⋅K) * (300.15 K) / (2.5 L)
Partial pressure of N2 = (0.25 mol) * (0.0821 L⋅atm/mol⋅K) * (300.15 K) / (2.5 L)
Now, let's calculate the total pressure exerted by each gas:
Total pressure exerted by SO2 = partial pressure of SO2
Total pressure exerted by N2 = partial pressure of N2
Finally, let's calculate the total pressure:
Total pressure = partial pressure of SO2 + partial pressure of N2
The law on which this calculation is based is known as Dalton's Law of Partial Pressures, which states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the individual partial pressures of each gas.
PV = nRT
P = total pressure
P x 2.5 = (0.25)2 x 0.83 x27
P= 4.482 degree celcius