HomeworkLib
Question

You have two moles of gaseous carbon dioxide at room temperature to which you add three...

You have two moles of gaseous carbon dioxide at room temperature to which you add three kilocalories of heat. a. What is its increase in temperature? b. What is its change in internal energy?

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

Homework Answers

Answer #1


internal energy E1 = (3/2)*n*R*T1


energy added = 3000 calorie = 3000*4.2 = 12600 J


total energy E2 = (3/2)*n*R*T2

E2 = E1 + 12600


E2 - E1 = 12600

(3/2)*2*8.314*dT = 12600


dT = 505 K


==================

change = 12600 J

0 0
Add a comment
Know the answer?
Add Answer to:
You have two moles of gaseous carbon dioxide at room temperature to which you add three...
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 cylinder contains 0.300 mol of carbon dioxide (CO2)gas at a temperature of 23.0 ∘C. The...

    A cylinder contains 0.300 mol of carbon dioxide (CO2)gas at a temperature of 23.0 ∘C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The cylinder is placed on a hot plate and a 920 J of heat flows into the gas, thereby raising its temperature to 130 ∘C. Assume that the CO2 may be treated as an ideal gas. 1. What is the change in internal energy of the...

  • Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 ...

    PART ONE: PART TWO: PART THREE: PART FOUR: Gaseous methane (CH4) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2 and gaseous water (H20). Suppose 13. g of methane is mixed with 13.8 g of oxygen. Calculate the minimum mass of methane that could be left over by the chemical reaction. Round your answer to 2 significant digits A 1.32-g sample of a compound is burned in a bomb calorimeter, producing a temperature change from 20.85 °C...

  • Consider a sample of carbon dioxide solid at room temperature and pressure. This substance will change...

    Consider a sample of carbon dioxide solid at room temperature and pressure. This substance will change from solid to a gas under these conditions. Which of the following is correct about this change of state? A) melting, exothermic B) melting, endothermic C) sublimation, exothermic D) sublimation, endothermic

  • A cylinder contains 0.250 mol of carbon dioxide (CO2) gas at a temperature of 27.0∘C. The...

    A cylinder contains 0.250 mol of carbon dioxide (CO2) gas at a temperature of 27.0∘C. The cylinder is provided with a frictionless piston, which maintains a constant pressure of 1.00 atm on the gas. The gas is heated until its temperature increases to 127.0∘C. Assume that the CO2 may be treated as an ideal gas. How much work W is done by the gas in this process? What is the change in internal energy ΔU of the gas? How much...

  • Your instructor gives you a 100 g of dry ice (solid carbon dioxide) at -100 °C....

    Your instructor gives you a 100 g of dry ice (solid carbon dioxide) at -100 °C. Through the course of an experiment, you end up with 100 g of gaseous carbon dioxide at 0 °C. Answer the following questions based on this data. Assume that no heat is lost to the outside environment during the experiment. The specific heats for solid and gaseous carbon dioxide are 0.296 and 0.203 cal/g-°C respectively. Remember, carbon dioxide sublimes from solid to gas at...

  • Consider a given volume of carbon dioxide gas at room temperature (20.00C). (Molar Mass of Carbon...

    Consider a given volume of carbon dioxide gas at room temperature (20.00C). (Molar Mass of Carbon dioxide is: 44.0 x 10-3 kg mol-1 J). (i). Calculate the root-mean-square Speed, Vrms, of a molecule of the gas?        The answer must be given in scientific notation and specified to an appropriate number of scientific figures. (ii). At what temperature would the root-mean-square-speed be half of that at room temperature?

  • Explain why Carbon Dioxide is a gas at room temperature while a diamond is a solid...

    Explain why Carbon Dioxide is a gas at room temperature while a diamond is a solid even though they both have covalent bonds.

  • At an atmospheric pressure of 1.01×105Pa, carbon dioxide (CO2) sublimes at a temperature of -78.5∘C. The...

    At an atmospheric pressure of 1.01×105Pa, carbon dioxide (CO2) sublimes at a temperature of -78.5∘C. The heat of sublimation is 5.71×105J/kg. You let heat flow into 6.0 kg of solid CO2 (volume 4.0×10−3m3) at atmospheric pressure and a constant -78.5∘C until it has completely sublimed to gas at -78.5∘C.The CO2 gas occupies a volume of 3.4 m3. A) For this process, calculate how much heat flows into the CO2. B) For this process, calculate how much work the CO2 does...

  • Question 2: (13 Marks) A quantity of carbon dioxide occupies a volume of 0.14 m'at 975...

    Question 2: (13 Marks) A quantity of carbon dioxide occupies a volume of 0.14 m'at 975 kPa and 370 °C. It is heated at constant volume to a pressure of 4.2 MPa, after which it is expanded in an insulated cylinder to a pressure of 270 kPa. Sketch these processes on a P-V diagram. Assuming Cp = 1.075 kJ/kg K for carbon dioxide, determine: A. The temperature at the start of the expansion B. The volume after expansion C. The...

  • An ideal gas mixture contains 4 moles of carbon dioxide and 8 moles of nitrogen. The...

    An ideal gas mixture contains 4 moles of carbon dioxide and 8 moles of nitrogen. The mixture is compressed adiabatically from100kPa and 20°C to 0.5 MPa. What is the final temperature of the gas mixture? Use second law word, entropy change.

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