A sample of nitrogen gas is heated to 100°C, at a pressure of 10kPa and volume of 0.2m^3. How many moles of gas are present?

In order to answer this question, the equation: PV=nRT must be used.P is pressure, V is volume, n is moles, R is the gas constant and T is temperature. Firstly the units in the question must be converted to SI units so they give the correct answer in the equation. Volume is correct in m^3, so this can be left. Temperature must be converted to kelvin by doing 273 + 100 = 373 K. 10 KPa must be converted into Pa by multiplying 10 by 1000, to give 10,000 K. The gas constant is 8.314 JK^-1mol^-1. PV=nRT can be rearranged to n=PV/RT. The new values can then be substituted into the equation, n=(10,000 Pa x 0.2 m^3)/(8.314 JK^-1mol^-1 x 373 K)= 0.645 moles of nitrogen gas.

Answered by Tara B. Chemistry tutor

9250 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What reaction occurs when benzene is mixed with equal amounts of sulphuric and nitric acid?


What is an enthalpy change?


Explain what is meant by optical isomerism.


Explain why fluorine is more reactive than chlorine.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2024

Terms & Conditions|Privacy Policy
Cookie Preferences