ZuoTi.Pro
Question

PRACTICE EXAMPLE A: A mixture of 0.197 mol CO2(g) and 0.00278 mol H2O(g) is held at 30.0 °C and 2.50 atm. What is the partial

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0.197 mol coleg 0.00278 mol lho cg) (Pt) Pressure of the mixture = 2.50 atm No to fal moles of gases = (0.197 +0.00276) mok 0Partial pressure of tha, PHO - H120 x = 0.10139x2.50 am - 0.03 a 75 atm partial Pressure of co2 = 2.46525 atm Postial Pressur

0 0
Add a comment
Know the answer?
Add Answer to:
PRACTICE EXAMPLE A: A mixture of 0.197 mol CO2(g) and 0.00278 mol H2O(g) is held at...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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

  • A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O...

    A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g)+H2(g)⇌CO(g)+H2O(g) Calculate the initial partial pressure of CO2. Calculate the initial partial pressure of H2. Calculate the initial partial pressure of H2O, H2 and CO2

  • A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O...

    A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO2(g)+H2(g)⇌CO(g)+H2O(g) A. Calculate the initial partial pressure of CO2CO2. Express your answer to three significant figures and include the appropriate units. B. Calculate the initial partial pressure of H2H2. Express your answer to three significant figures and include the appropriate units. C. Calculate the initial partial pressure of H2OH2O. Express...

  • 2. A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L system. The follo...

    2. A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L system. The following equilibrium is established at 500 K CO2(g) + H2(c) -> CO(S) + H2O(g) At equilibrium, Prao = 3.51 atm. A) Calculate the equilibrium partial pressures of CO2. Hz, and CO (6 points) and B) Calculate Kfor the reaction (4 points). Recall PV = nRT, with R = 0.0821 L-atm/mol-K. Hint: ICE chart not necessary. Notice...

  • A gas mixture is made up of O2 (8.14 g), N2 (7.15 g), and CO2 (15.3...

    A gas mixture is made up of O2 (8.14 g), N2 (7.15 g), and CO2 (15.3 g). The mixture has a volume of 25.2 L at 74 °C. Calculate the partial pressure of each gas in the mixture and the total pressure of the gas mixture. PO2 = atm PN2 = atm PCO2 = atm Ptotal = atm

  • A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at...

    A mixture of CS2(g) and excess O2(g) is placed in a 10 L reaction vessel at 100.0 ∘C and a pressure of 3.20 atm . A spark causes the CS2 to ignite, burning it completely, according to the equation: CS2(g)+3O2(g)→CO2(g)+2SO2(g) After reaction, the temperature returns to 100.0 ∘C, and the mixture of product gases (CO2, SO2, and unreacted O2) is found to have a pressure of 2.50 atm . What is the partial pressure of each gas in the product...

  • A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of...

    A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 8.00 L vessel at 27.00°C. A) What is the total pressure in the vessel (atm)? B) What is the pressure (atm) of H2? C) What is the pressure (atm) of N2? D) What is the pressure (atm) of CH4?

  • If a gaseous mixture is made by combining 4.68 g Ar and 2.73 g Krin an evacuated 2.50 L container at 25.0 °C, what...

    If a gaseous mixture is made by combining 4.68 g Ar and 2.73 g Krin an evacuated 2.50 L container at 25.0 °C, what are the partial pressures of each gas, PA and Pr, and what is the total pressure, Poul exerted by the gaseous mixture? Par = 0.423 am Pk 0.200 atm Potal = 0.623 A 7.85 L container holds a mixture of two gases at 43 °C. The partial pressures of gas A and gas B, respectively, are...

  • A tank contains a mixture of 48.2 g of oxygen gas and 70.0 g of carbon...

    A tank contains a mixture of 48.2 g of oxygen gas and 70.0 g of carbon dioxide gas at 23 °C. The total pressure in the tank is 8.40 atm. Calculate the partial pressure (in atm) of each gas in the mixture. Partial pressure = atm O2 Partial pressure = atm CO2 What mass of neon gas is required to fill a 8.00 L container to a pressure of 1.42 atm at 18 °C? Mass = g Ne How many...

  • Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g)CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611Kp=0.0611 at 2000 KK A reaction mixture initially contains a COCO...

    Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g)CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0.0611Kp=0.0611 at 2000 KK A reaction mixture initially contains a COCO partial pressure of 1354 torrtorr and a H2OH2O partial pressure of 1756 torrtorr at 2000 KK. A) Calculate the equilibrium partial pressure of CO2CO2 . B) Calculate the equilibrium partial pressure of H2H2.

  • A 0.357 mol sample of CO2(g), initially at 298 K and 1.00 atm, is held at...

    A 0.357 mol sample of CO2(g), initially at 298 K and 1.00 atm, is held at constant pressure while enough heat is applied to raise the temperature of the gas by 18.9 K. Calculate the amount of heat ? required to bring about this temperature change, and find the corresponding total change in the internal energy Δ? of the gas. Assume that the constant‑pressure molar specific heat for CO2(g), which consists of linear molecules, is equal to 7?/2, where ?...

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