50 points plus brainliest!!
1.)Boyle’s law is
P1V1 = P2V2
A balloon has an initial volume of 355 L and an initial pressure of 234 kPa. The volume is lowered to a final value of 227 L. Use Boyle's Law to calculate the final pressure.
Round to two decimal points and do not use units.
2.)The ideal gas law equation is
PV=nRT.
How many moles of gas are in a closed container with a pressure of 400 kPa, volume of 10 L and a temperature of 450 K?
Use 8.31 for R
Round to two decimal places and do not use units.
Answers: 3
Chemistry, 21.06.2019 23:30, 23gordns
Problem #3 (ch. 1, problem 15)the ideal gas law provides one way to estimate the pressure exerted by a gas on a container. the law isí‘ťí‘ť=푛푛푛푛푛푛푉푉mo re accurate estimates can be made with the van der waals equationí‘ťí‘ť=í‘›í‘›í‘›í‘›í‘›í‘›í‘ ‰í‘‰â’푛푛푟푟â’푞푞푛푛2í‘ ‰í‘‰2where the term nb is a correction for the volume of the molecules and the term an2/v2is a correction for molecular attractions. the values of a and b depend on the type of gas. the gas constant is r, the absolutetemperature is t, the gas volume is v, and the number of moles of gas molecules is indicated by n. if n = 1 mol of an ideal gas were confined to a volume of v = 22.41 l at a temperature of 0â°c (273.2k), it would exert a pressure of 1 atm. in these units, r = 0.0826.for chlorine gas (cl2), a = 6.49 and b = 0.0562. compare the pressure estimates given by the ideal gas law and the van der waals equation for 1 mol of cl2 in 22.41 l at 273.2 k. what is the main cause of the difference in the two pressure estimates, the molecular volume or the molecular attractions?
Answers: 1
50 points plus brainliest!!
1.)Boyle’s law is
P1V1 = P2V2
A balloon has an initia...
P1V1 = P2V2
A balloon has an initia...
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