in a ten litre vessle ,the total pressure of a gaseous mixture containing H2,N2 are 3.7 and 4.2 atm , respectively . the partial pressure of CO2 is ….

To find the partial pressure of CO2 in a gaseous mixture, we can use Dalton's Law of Partial Pressures. This law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture. In your case, we know the total pressures of H2 and N2, and we need to determine the partial pressure of CO2.

Understanding the Given Information

We have the following data:

• Total pressure of H2 = 3.7 atm
• Total pressure of N2 = 4.2 atm
• Volume of the vessel = 10 liters (though this is not directly needed for calculating partial pressures)

Applying Dalton's Law

According to Dalton's Law, the total pressure (P_total) of the gas mixture can be expressed as:

P_total = P_H2 + P_N2 + P_CO2

Where:

• P_H2 is the partial pressure of hydrogen
• P_N2 is the partial pressure of nitrogen
• P_CO2 is the partial pressure of carbon dioxide

Calculating the Total Pressure

First, we need to find the total pressure of the mixture. Since we have the partial pressures of H2 and N2, we can add them together:

P_total = P_H2 + P_N2 = 3.7 atm + 4.2 atm = 7.9 atm

Finding the Partial Pressure of CO2

Now, if we assume that the total pressure of the system is equal to the sum of the partial pressures of the gases present, we can rearrange the equation to find the partial pressure of CO2:

P_CO2 = P_total - (P_H2 + P_N2)

Substituting the values we have:

P_CO2 = 7.9 atm - (3.7 atm + 4.2 atm)

P_CO2 = 7.9 atm - 7.9 atm = 0 atm

Conclusion

From our calculations, the partial pressure of CO2 in this mixture is 0 atm. This indicates that there is no CO2 present in the gaseous mixture, as the total pressure is fully accounted for by the hydrogen and nitrogen gases. If you have any further questions or need clarification on any part of this process, feel free to ask!