REFER TO THESE WORKED EXAMPLES AS YOU ATTEMPT TO SOLVE YOUR PROBLEM: If a gas is cooled from 323 K to 273 K and the volume is kept constant, Example: what final pressure would result if the original pressure was 755 mm Hg? P1 = 755 mm Hg T1 = 323 K P2 = ??? T2 = 273 K 1. 2. Identify givens and the unknown. Convert all temperatures to Kelvin. 3. Rearrange the equation if you'd like. Substitute values into the equation. 5. Solve for the unknown. 4. 6. Check your answer against theory. P₁ = P₂ Т1 Т2 Support your calculations with reasoning using the concept of Gay-Lussac's Law here. P1 T1 755 mm Hg 323 K P2 T2 P2 273 K P2 * 323 K 223 K 755 mm Hg * 273 K 323 K 638 mm Hg = P2 If a gas in a closed container is pressurized from 19 atm to 23 atm and its original temperature was 35 C, what would be the final temperature of the gas? Show your calculations here.

REFER TO THESE WORKED EXAMPLES AS YOU ATTEMPT TO SOLVE YOUR PROBLEM: If a gas is cooled from 323 K to 273 K and the volume is kept constant, Example: what final pressure would result if the original pressure was 755 mm Hg? P1 = 755 mm Hg T1 = 323 K P2 = ??? T2 = 273 K 1. 2. Identify givens and the unknown. Convert all temperatures to Kelvin. 3. Rearrange the equation if you'd like. Substitute values into the equation. 5. Solve for the unknown. 4. 6. Check your answer against theory. P₁ = P₂ Т1 Т2 Support your calculations with reasoning using the concept of Gay-Lussac's Law here. P1 T1 755 mm Hg 323 K P2 T2 P2 273 K P2 * 323 K 223 K 755 mm Hg * 273 K 323 K 638 mm Hg = P2 If a gas in a closed container is pressurized from 19 atm to 23 atm and its original temperature was 35 C, what would be the final temperature of the gas? Show your calculations here.

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

Use the ideal gas law to verify the triple product rule.
please help me, double check your answers previous tutors got it wrong.
2. For each of the following sets of data, calculate the missing quantity. Assume that the amount of gas remains constant. SHOW WORK a. V = 8.45 L, at 1.64 atm and 32.0 °C; V = 6.15 L, at ? _atm and 32.0 °C. b. V = 5.82 L, at 1.09 atm and 21.0 °C; V = ? , at 2.75 atm and 45.0 °C.
&drc-D0&gi-24758088- A flexible lighting fixture is filled with neon. The starting volume of the fixture is 8.2L and the pressure of the neon is 3.2 atm. If the fixture is compressed, reducing the volume to 1.6L, what is the new pressure in the lamp? Your Answer: Answer units D Add attachments to support your work
need help with this question please teacher didn’t explain well
5.- Nitrogen gas occupies a volume of 4.30 L at 54°C. If its volume increased to 7.80 L at the same pressure. Calculate the final temperature in kelvin. 235k 2k 593.163k 334.43k 200k
Please answer the question Below.
a. Given the following set of values for a gas, calculate the unknown quantity: P = 743.3 mm Hg V = ? L n = = 0.1021 mol T = 23.3 °C V = L b. Given the following set of values for a gas, calculate the unknown quantity: P = ? atm V = 28.4 mL n = 0.007052 mol T = 20.5 °C P = c. Given the following set of values for a gas, calculate the unknown quantity: P= 1.079 atm T = atm V = 44.7 mL n = 0.003411 mol T = ? K K
7. When detern ing the mass of a liquid, ras in a hurry and did not allow enough time for the temperature of the flask to reach the temperature of the boiling water bath. The student recorded the temperature of the gas as 100.0°C when it was only 80.0°C, Is the molar mass calculated by the student higher or lower than the accepted molar mass, or does this error have no effect on the calculated result? Briefly explain your answer # 2/HB Office DEPOTS b) If the student assumed the volume of the flask was 125 mL (as marked by the side of the flask) rather than measuring the volume experimentally, would the unknown's calculated molar mass be too high, too low, or unaffected? Explain. # 2/HB 4