At a constant temperature, an ideal gas is compressed from 6,0 Liters to 4,0 Liters by a constant external pressure of 5.00 atm. 1 atm =1.01 x 10° Pa Answer the following questions by filling in the blanks a. What is the constant external pressure applied to the gas in Pa? Represent your answer with 3 significant figure using scientific notation, without units.e.g. 1.23E+3 The external presure applied to the gas is Pa b. What is the change in volume of the gas in Liters? Represent your answer with 1 decimal place using normal notation, without units. The change in volume of the gas is c. What is the change in volume of the gas in m3? Represent your answer with 3 significant figure using normal notation, without units. m3 The change in volume of the gas is

At a constant temperature, an ideal gas is compressed from 6,0 Liters to 4,0 Liters by a constant external pressure of 5.00 atm. 1 atm =1.01 x 10° Pa Answer the following questions by filling in the blanks a. What is the constant external pressure applied to the gas in Pa? Represent your answer with 3 significant figure using scientific notation, without units.e.g. 1.23E+3 The external presure applied to the gas is Pa b. What is the change in volume of the gas in Liters? Represent your answer with 1 decimal place using normal notation, without units. The change in volume of the gas is c. What is the change in volume of the gas in m3? Represent your answer with 3 significant figure using normal notation, without units. m3 The change in volume of the gas is

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...

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Answer part a and b
2 n The van der Waals equation of state. R stands for the gas constant and n for moles of p+a v2 (V-nb)=nRT gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. x10 What are the units of a? What are the units of b? For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. || atm Use the van der Waals equation to calculate the pressure of a sample of water at 500.0 °C with a molar volume of 0.366 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. | atm
Calculate the mass of the air in a typical hot-air balloon that would have a volume of 5.00 x 10° mL when the temperature of the gas is 303 K and the pressure is 0.984 atm. Assume that the average molecular weight of air is 29.0 g/mol. (show your calcuations) Equations: PV=nRT; R=0.08206 L-atm/mol-K B IU 0/10000 Word Limit 23 24 25 26 27 28 29 30 31 32 ENM
Use the van der Waals equation of state to calculate the pressure of 3.30 mol of HI at 483 K in a 4.60 L vessel. Van der Waals constants can be found in the van der Waals constants table. P = atm Use the ideal gas equation to calculate the pressure under the same conditions. P = atm Under these conditions, would you expect HI or CCl, to deviate more from ideal behavior? Why? CCl because it occupies a larger volume and it has smaller dispersion forces between molecules. HI because it occupies a smaller volume and it has smaller dispersion forces between molecules. HI because it occupies a larger volume and it has smaller dispersion forces between molecules. CCI, because it occupies a larger volume and it has greater dispersion forces between molecules. HI because it occupies a smaller volume and it has greater dispersion forces between molecules. CCI, because it occupies a smaller volume and it has greater dispersion forces between molecules.
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#4 part a.)Calculate vol in L
Several years ago there was a big controversy in football that needed chemistry tosolve it! In “Deflategate”, the problem was a lack of understanding of the ideal gaslaw. Use the following data to determine the final gauge pressure of one of thefootballs from that event. If the football was initially inflated to 12.50 psig in thelocker room at 69.0 F, what gauge pressure would it be when the football wastaken to the field at 48.0 F? Atmospheric pressure = 12.30 psi that day.
Consider the two flasks joined together with a stopcock (shown in the diagram below). Calculate the final partial pressure contributed by each gas to the mixture when the stopcock connecting the flasks is opened. (Assume the total volume is 6 L). 4 1 L of N₂ at 303000 Pa 5 L of H₂ at 101000 Pa a. рH₂= 84167 Pa, pN₂ = 50500 Pa = рн₂ 101000 Pa, pN₂= 101000 Pa рH₂=50500 Pa, pN₂ = 84167 Pa рн₂= 134667 Pa, pN₂ = 50500 Pa e. рH₂= 84167 Pa, pN₂ = 134667 Pa оооо O b. OC. O d.
*00 LL L山 A sample of an unknown compound is vaporized at 180. °C. The gas produced has a volume of 2410. mL at a pressure of 1.00 atm, and it weighs 2.08 Assuming the gas behaves as an ideal gas under these conditions, calculate the molar mass of the compound. Round your answer to 3 significant digits. OU mol 5. Continue Submit Assignmen O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center | Accessibility MacBook Pro F3 F5 F7 F8 F10 64 $4 # 5. R. B option command command option
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A helium-filled balloon accidentally floats to the ceiling. The balloon is initially inflated to a radius of 6 inches (assume a sphere). The balloon’s empty mass is 10 g. The density of the rubber is 0.8 g/cm3. The contents of the balloon are purely helium @ p=1 atm, T=300 K. Assume that D=3.00E-8 kg/m2s and assume the pressure inside the balloon does not change much. Calculate the time required for the balloon to start to sink on its own, because of diffusion.