A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 3 years ago
After 1.00 ml of water is completely vaporized to gas, how many milliliters of vapor are produced at standard temperature and pressure? (Density of water is 1.00 g/mL; molar volume of any gas at STP is 22.4 L/mol.)
anonymous
 3 years ago
After 1.00 ml of water is completely vaporized to gas, how many milliliters of vapor are produced at standard temperature and pressure? (Density of water is 1.00 g/mL; molar volume of any gas at STP is 22.4 L/mol.)

This Question is Open

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0I think you must first find moles of water (n) in 1 ml of water, the apply PV=nRT.

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0density=mass/volume. given that 1 ml of water is vaporized therefore we calculate the mass of water that has been vaporized which comes out to be 1 g. now we calculate no of moles of water vaporized i.e. n= 1/18. (molar mass of water =18 g). Use PV=nRT to calculate V.
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.