Answered

Get the most out of your questions with the extensive resources available on IDNLearn.com. Ask your questions and receive comprehensive, trustworthy responses from our dedicated team of experts.

What is the total pressure exerted by a mixture of 48.0 grams of CH4 and 56.0 grams of
hydrogen gas when confined in a volume of 15.0 liters at 13°C.

Sagot :

Pstnonsonjokuidn

The pressure of the gas is obtained as 48 atm.

What is the total pressure?

Now we know that;

Number of moles of CH4 = 48.0 grams /16 g/mol = 3 moles

Number of moles of H2 =  56.0 grams/2 g/mol = 28 moles

Total number of moles present = 3 moles + 28 moles = 31 moles

Using;

PV =nRT

P = total pressure

V = total volume

n = total number of moles

R = gas constant

T = temperature

P = nRT/V

P = 31 * 0.082 * 286/15

P = 48 atm

Learn more about pressure of a gas:https://brainly.com/question/18124975

#SPJ1

Thank you for using this platform to share and learn. Don't hesitate to keep asking and answering. We value every contribution you make. Your search for answers ends at IDNLearn.com. Thanks for visiting, and we look forward to helping you again soon.