4g of h2 and 32g of so2 are present in gaseous mixture at n.t.p the partial pressure of h2 is?
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To find the partial pressure of hydrogen gas (H2) in the given gaseous mixture at N.T.P (Normal Temperature and Pressure), we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
First, we need to calculate the number of moles of H2 and SO2 using their respective molar masses. The molar mass of hydrogen gas (H2) is 2 g/mol, and the molar mass of sulfur dioxide (SO2) is 64 g/mol.
Number of moles of H2 = Mass of H2 / Molar mass of H2
= 4 g / 2 g/mol
= 2 mol
Number of moles of SO2 = Mass of SO2 / Molar mass of SO2
= 32 g / 64 g/mol
= 0.5 mol
Now, since the given gaseous mixture is at N.T.P, we know that the volume and temperature will be constant. Therefore, we can assume that the volume (V) and temperature (T) are constant.
Now, using the given values, we can calculate the partial pressure of hydrogen gas.
Let's assume the total pressure of the mixture is Ptotal.
According to Dalton's law of partial pressures, the total pressure is the sum of the partial pressures of the individual gases:
Ptotal = PH2 + PSO2
Given that the number of moles of H2 is 2 and the number of moles of SO2 is 0.5, we can substitute the values into the equation:
Ptotal = (2/2) * PH2 + (0.5/2) * PSO2
Ptotal = PH2 + 0.25 * PSO2
Since the total pressure is equal to the pressure of the mixture at N.T.P, which is 1 atm, we can substitute Ptotal with 1 atm:
1 atm = PH2 + 0.25 * PSO2
Now, we have the equation for the total pressure in terms of the partial pressures of the gases H2 and SO2.
To find the partial pressure of H2, substitute the given values:
1 atm = PH2 + 0.25 * PSO2
1 atm = PH2 + 0.25 * (Ptotal - PH2)
Simplifying the equation:
1 atm = PH2 + 0.25 * Ptotal - 0.25 * PH2
Combining like terms:
0.75 * PH2 = 1 atm - 0.25 * Ptotal
0.75 * PH2 = 1 atm - 0.25 * 1 atm (since Ptotal = 1 atm)
0.75 * PH2 = 1 atm - 0.25 atm
0.75 * PH2 = 0.75 atm
Now, we can isolate PH2 by dividing both sides of the equation by 0.75:
PH2 = (0.75 atm) / (0.75)
PH2 = 1 atm
Therefore, the partial pressure of hydrogen gas (H2) in the given gaseous mixture at N.T.P is 1 atm.
To find the partial pressure of H2 in the gaseous mixture, we need to use the concept of mole fraction and Dalton's Law of Partial Pressures.
1. Calculate the number of moles of H2 and SO2:
Number of moles of H2 = mass of H2 / molar mass of H2
Number of moles of H2 = 4 g / 2 g/mol (molar mass of H2 = 2 g/mol)
Number of moles of H2 = 2 mol
Number of moles of SO2 = mass of SO2 / molar mass of SO2
Number of moles of SO2 = 32 g / 64 g/mol (molar mass of SO2 = 64 g/mol)
Number of moles of SO2 = 0.5 mol
2. Calculate the total number of moles of gas in the mixture:
Total number of moles = Number of moles of H2 + Number of moles of SO2
Total number of moles = 2 mol + 0.5 mol
Total number of moles = 2.5 mol
3. Calculate the mole fraction of H2:
Mole fraction of H2 = Number of moles of H2 / Total number of moles
Mole fraction of H2 = 2 mol / 2.5 mol
Mole fraction of H2 = 0.8
4. Use Dalton's Law of Partial Pressures:
According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each gas.
Since we are given that the gaseous mixture is at NTP (normal temperature and pressure), the total pressure is 1 atm.
Partial pressure of H2 = Mole fraction of H2 * Total pressure
Partial pressure of H2 = 0.8 * 1 atm
Partial pressure of H2 = 0.8 atm
Therefore, the partial pressure of H2 in the gaseous mixture at NTP is 0.8 atm.