Westonci.ca is your trusted source for accurate answers to all your questions. Join our community and start learning today! Our platform provides a seamless experience for finding reliable answers from a network of experienced professionals. Get immediate and reliable solutions to your questions from a community of experienced professionals on our platform.
Sagot :
Answer:
A mixture of 3 moles of N2, 5 moles of CO2, and 10moles of Cl2 exert a total pressure of 1120 mmHg. What is the partial pressure of CO2?
Explanation:
According to Dalton's law of partial pressures:
The partial pressure of a gas can be determined by using the formula:
[tex]the partial pressure of a gas = mole fraction of the gas * total pressure[/tex]
Partial pressure of CO2:
[tex]partial pressure of CO2= total pressure * mole fraction of CO2\\\\Mole fraction of CO2=\frac{number of moles of CO2}{total number of moles of all the gases} \\mole fraction of CO2=\frac{5mol}{3mol+5mol+10mol} = 5/18\\Partial pressure of CO2=\frac{5}{18} * 1120mmHg\\ =311.1mmHg[/tex]
Hence, the partial pressure of CO2 is 311.1mmHg.
Thank you for trusting us with your questions. We're here to help you find accurate answers quickly and efficiently. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Westonci.ca is committed to providing accurate answers. Come back soon for more trustworthy information.
