**Question:** As described in the video, which gas law predicts the relationship between volume and pressure?[Input Box] (Note: There are no graphs or diagrams in the image to explain.) ### Problem StatementA sample of krypton gas occupies 5.00 L at 4.89 atm. What volume does the gas occupy at 10.4 atm?Assume T and n are constant.*Make sure you type in your answer with the correct sig figs and a unit.*### Instructions- Calculate the new volume of krypton gas using the principles of gas laws, specifically Boyle’s Law, which states that $ P_1 \times V_1 = P_2 \times V_2 $.- Input your answer in the provided space, ensuring that you maintain the correct significant figures and include the appropriate unit (liters).### GuidanceFor this task, recall how pressure and volume are inversely related when temperature and number of moles are constant. Use the known values:- Initial Volume $ V_1 = 5.00 \, \text{L} $- Initial Pressure $ P_1 = 4.89 \, \text{atm} $- Final Pressure $ P_2 = 10.4 \, \text{atm} $Calculate for the final Volume $ V_2 $.

We are to discuss which gas law gives the relation between pressure and volume. also, we have V1 = 5.00 L, P1 = 4.89 atm V2 = ? and P2 = 10.4 atm, we are to find the volume V2.Boyle's law gives the relation between pressure and volume. It states that at a constant temperature, the volume of a gas is inversely proportional to it's pressure. P ∝ 1/V or, PV = constant or, P1V1 = P2V2Now we have the relation P1V1 = P2V2 putting the given values, 4.89× 5.00 = 10.4×V2 V2 = 2.35 L Hence, volume at 10.4 atm is 2.35 L.

Answered: A sample of krypton gas occupies 5.00 L…

Science

Chemistry

A sample of krypton gas occupies 5.00 L at 4.89 atm. What volume does the gas occupy at 10.4 atm? Assume T and n are constant. Make sure you type in your answer with the correct sig figs and a unit.

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

A sample of oxygen gas has a density of g/L at a pressure of 1.04 atm and a temperature of 50.0 °C. Assume ideal behavior.
If 9.00 g helium gas is added to a 1.00 L balloon containing 1.00 g of helium gas, what is the new volume of the balloon? Assume no change in temperature or pressure. Enter your answer in the box provided. L.
A.) a mixture of argon and neon gases, in a 8.32 L flask at 21 degrees Celsius, contains 15.3 grams of argon and 2.24 grams of neon. The partial pressure of neon in the flask is ____atm and the total pressure in the flask is ____atm. B.) a mixture of helium and xenon gases is maintained in a 9.17 L flask at a pressure of 1.28 atm and a temperature of 84 degrees Celsius. If the gas mixture contains 0.637 grams of helium, the number of grams of xenon in the mixture is ____grams.
CLESS the soction in your e lext. Part A What is the pressure in millimeters of mercury of 0.0125 mol of helium gas with a volume of 213 mL at 40. °C? (Hint: You must convert each quantity into the correct units (L, atm, mol, and K) before substituting into the ideal gas law.) Express your answer with the appropriate units. Value Units Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remalining Next > Provide Feedback MacBook Air F7 吕口 F3 esc * & $ % 9 @ # 6 3 4 P T Y E R Q G
A mixture of neon and hydrogen gases at a total pressure of 973 mm Hg contains neon at a partial pressure of 331 mm Hg. If the gas mixture contains 2.39 grams of neon, how many grams of hydrogen are present?
A sample of xenon gas occupies 71.1 litres under a pressure of 1.55 x 103 torr at 25.0 °C. What volume (in litres) would this sample occupy at -72.8 °C, if the pressure remained constant? Assume xenon acts as an ideal gas. Enter the numerical value (no units), using 3 significant figures. Type your answer...
If an ideal gas has a pressure of 1.37 atm,1.37 atm, a temperature of 467 K,467 K, and a volume of 98.91 L,98.91 L, how many moles of gas are in the sample?
Since the volume of one mole of any gas at STP is 22.7 L, the density of one mole of any gas at STP is a constant value. Do you agree or disagree with this statement? Why?
A 33.9−L volume of methane gas is heated from 28°C to 69°C at constant pressure. What is the final volume of the gas?
If 0.00901 mole of neon gas at a particular temperature and pressure occupies a volume of 242 mL, what volume of 0.00703 mole of neon occupy under the same conditions?