Gas is trapped inside of a cell with volume 150 m3. The gas exerts 7300 Pa of pressure against the walls of the cell. A machine then expands the cell and gives off 290 kJ of heat to the gas during the process. If the internal energy changed by 97 kJ, what is the final volume of the cell? Assume the pressure stays constant. 120 m3 210 m3 97 m3 180 m3 200 m3

Gas is trapped inside of a cell with volume 150 m3. The gas exerts 7300 Pa of pressure against the walls of the cell. A machine then expands the cell and gives off 290 kJ of heat to the gas during the process. If the internal energy changed by 97 kJ, what is the final volume of the cell? Assume the pressure stays constant. 120 m3 210 m3 97 m3 180 m3 200 m3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Assuming constant pressure, a gas has a final volume of 15 L. If the temperature increases from 330 K to 450 K, find the initial volume. Show all work in the space provided, and then write your final answer on the short line.
A 325 g piece of unknown metal is boiled. The metal is then soaked in 500 g of water at 20 ° C. If the final temperature of the mixture is 30 ° C., what is the thermal capacity of the metal?
What amount of heat is required to convert 10.9 g of an unknown liquid (MM 83.21 g/mol) at 19.2°C to a gas at 93.5 °C? (heat capacity of iquid 1.58 J/g.C; heat capacity of gas 0.932 JIg.°C; AHvap 22.5kJ/mol, Tb= 57.3°C) kJ
A hot, 3.00 g metal ball at 140.oC was placed in 8.0 mL of cold water at 12oC. The specific heat capacity of the metal is 3.3 J/g◦C. What was the final temperature of the water? [Hint: Look up the density of water.]
1a. Calculate the pressure of a sample of 1 mole of argon gas in a 0.1500 L flask at -10.2 ℃ using the ideal gas law and the Van der Waals equation. The a value for argon is 1.34 (L 2 ∙ atm/mol2 ) and the b value is 0.0322 (L/mol). Show all work Ideal pressure= ? real pressure =? 1b.Why is there a difference in the real gas pressure and the ideal pressure? Explain what assumption(s) of the kinetic molecular theory of gases break down under these conditions.
Please don't provide handwritten solution ....
How much energy is required to raise the temperature of 12.2 grams of gaseous nitrogen from 23.0 °C to 37.0 °C ?
Compared to 1 mole gas molecule at 25 °C, which of the following descriptions is true about 1 mole gas molecule at 400 °C? Broader distribution of molecular velocities Lower entropy Less number of microstates Less molecular motion
1. The formation of gaseous phosphorus trichloride is shown below: P4 (g) + 6 Cl2 (g) → 4 PCl3 (g) ΔH = -1207 kJ/mol If 4.30 kJ of heat are released as the formation reaction above proceeds, how many milliliters of gaseous phosphorus trichloride, measured at 35°C and 712 torr, will be produced?
What is kinetic energy of one mole of an ideal gas st 25C?
Ancient Romans built often out of bricks and mortar. A key ingredient in their mortar was quicklime (calcium oxide), which they produced by roasting limestone (calcium carbonate). 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid calcium carbonate (CaCO2) into solid calcium oxide and gaseous carbon dioxide. C 2. Suppose 86.0 L of carbon dioxide gas are produced by this reaction, at a temperature of 260.0 °C and pressure of exactly 1 atm. Calculate the mass of calcium carbonate that must have reacted. Round your answer to 3 significant digits.