Derive a gas law formula for a specific scenario One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 bar and a temperature of 273 K. The temperature is then increased to 308 K, but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,v,T).

Derive a gas law formula for a specific scenario One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 bar and a temperature of 273 K. The temperature is then increased to 308 K, but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,v,T).

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

With a graph please thank you!
There are 4.00 moles of gas in a sealed container with a volume of 3.00L. Some of the gas is removed while the temperature and pressure are held constant such that the final number of moles is 1.87. What is the fınal volume of the system?
Consider the following balanced chemical equation. 5 F2 (g) + Br2 (l) → 2 BrF5 (l) 0.789 atm of F2 in a 0.1250 L container at 26.5 °C reacted. How many mol of BrF5 were formed? SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank. Calculate the mol of F2 reacted (enter value only, with proper s.f.). mol Use the three blanks to enter the number, unit, and substance (in this order) that appears in the denominator of the…
The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).
A 1.56 mol sample of O2 gas is confined in a 37.6 liter container at 20.9 °C. If 1.56 mol of H2 gas is added and the volume and temperature of the system are held constant, explain in at least one sentence what will happen to... a. The average molecular speed of the system. In your answer, you should indicate whether the average molecular speed will increase, decrease or remain the same, and also indicate your reasoning why. b. The average kinetic energy of the system. In your answer, you should indicate whether the average kinetic energy will increase, decrease or remain the same, and also indicate your reasoning why.
Pls help me with the following asap and make sure its 100% correct, thanks
#4
Use 1 decimal point for all atomic weights (X.X). For the following oxygen, nitrogen, and helium mixture, determine the partial pressure of nitrogen if the gas is 101 g of oxygen, 286 g of nitrogen, and 502 g of helium at a total pressure of 400.0 kPa. ? kPa? I put 29.6, then 30 kPa both wrong... ....but don't know why... here is my work O=101/32=3.16, N=286/28=10.21, H=502/4=125.5 Total mol: 138.87 O 3.16/138.87=0.023 N: 10.21/138.87=0.074 H: 125.5/138.87= 0.90 0.074 (N) * 400 kPa= 29.6 kPa
Part 1. Determine the molar mass of a 0.314-gram sample of gas having a volume of 1.6 L at 287 K and 0.92 atm. Show your work.Part 2. Describe the temperature and pressure conditions at which the gas behaves like an ideal gas.
Consider the lungs, which can be modeled on a very basic level as a 5.0 L container of a mixture of N2 and O2 gases at 298 K. a) Calculate the pressure inside your lungs if filled with 0.15 mol the gas mixture described above, assuming it behaves ideally. b) Is it reasonable to assume that this gas mixture behaves ideally under these conditions? Why or why not?