Question

O GASES Calculating mole fraction in a gas mixture A 8.00 L tank at 19.8 °C is filled with 11.0 g of chlorine pentafluoride gas and 7.97 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Be sure each of your answer entries has the correct number of significant digits. mole fraction gas chlorine pentafluoride boron trifluoride
0 0
Add a comment Improve this question Transcribed image text
Answer #1

The Mo The tuo comfonds moleh mass to derehin homen moleeach ha. mole Gfs o 08Y33 molex CAF^ Therefsr GIFć δ.OBY 33 mole ole

Add a comment
Know the answer?
Add Answer to:
O GASES Calculating mole fraction in a gas mixture A 8.00 L tank at 19.8 °C...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • ANSWER NEEDS TO BE IN 3 SIGNIFICANT FIGURES O GASES Calculating partial pressure in a gas...

    ANSWER NEEDS TO BE IN 3 SIGNIFICANT FIGURES O GASES Calculating partial pressure in a gas mixture A 7.00 L tank at 6.66 °C is filled with 7.88 g of chlorine pentafluoride gas and 7.24 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction:...

  • Calculating partial pressure in a gas mixture A 8.00 L tank at 3.01 °C is filled...

    Calculating partial pressure in a gas mixture A 8.00 L tank at 3.01 °C is filled with 2.19 g of carbon dioxide gas and 4.83 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: carbon dioxide partial pressure 1x S ? mole fraction: chlorine...

  • A 5.00 L tank at 6.27 °C is filled with 3.97 g of dinitrogen difluoride gas...

    A 5.00 L tank at 6.27 °C is filled with 3.97 g of dinitrogen difluoride gas and 3.91 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. dinitrogen difluoride partial pressure: 0. sulfur tetrafluoride partial pressure: X 5 ? Total pressure in tank: atm A 8.00 L...

  • Calculating mole fraction in a gas mixture A8.00 L tank at 24.0 °C is filled with 18.2 g of sulfur tetrafluoride ga...

    Calculating mole fraction in a gas mixture A8.00 L tank at 24.0 °C is filled with 18.2 g of sulfur tetrafluoride gas and 7.54 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. mole fraction X 5 ? sulfur tetrafluoride boron t oride

  • O GASES Calculating mole fraction in a ges mbxture Christo A 10.00 L tank at 10.4...

    O GASES Calculating mole fraction in a ges mbxture Christo A 10.00 L tank at 10.4 °C is filled with 3.99 g of sulfur hexafluoride gas and 14.6 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. mole fraction gas ? X sulfur hexafluoride chlorine pentafluoride

  • Calculating partial prescure in a gas mixture A 6.00 L tank at 17.8 °C is filled...

    Calculating partial prescure in a gas mixture A 6.00 L tank at 17.8 °C is filled with 7.95 g of boron trifluoride gas and 5.67g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits mole fraction: alb boron trituoride partial pressure: mole fraction: partial pressure...

  • A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas...

    A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas and 5.50 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: dinitrogen difluoride partial pressure: atmx ? mole fraction: chlorine pentafluoride partial pressure: | atm Total...

  • A 8.00 L tank at 10.2 °C is filled with 8.47 g of chlorine pentafluoride gas...

    A 8.00 L tank at 10.2 °C is filled with 8.47 g of chlorine pentafluoride gas and 12.1 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: | atm x 6 ? mole fraction: carbon dioxide partial pressure:...

  • A 10.0 L tank at 23.4 °C is filled with 8.30 g of boron trifluoride gas...

    A 10.0 L tank at 23.4 °C is filled with 8.30 g of boron trifluoride gas and 9.63 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. :!! mole fraction: сто boron trifluoride ole partial pressure: atm Х ? AN mole fraction: chlorine pentafluoride partial pressure:...

  • A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas...

    A 8.00 L tank at 2.64 °C is filled with 9.82 g of chlorine pentafluoride gas and 10.1 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. mole fraction: chlorine pentafluoride partial pressure: atm x 6 ? mole fraction: dinitrogen difluoride partial pressure: atm...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT