Marcus measured the masses and volumes of samples of four different substances, and he calculated their densities. The table shows Marcus’s measured and calculated values. Substance Mass (g) Volume (cm3) Density (g/cm3)
aluminum 5.7 2.1 2.7
copper 14.4 1.6 9.0
iron 9.5 1.2 7.9
titanium 8.6 1.8 4.8

Next, Marcus obtained another sample, which is made of one of the four substances that he had already measured. The table shows Marcus’s measured values for this unknown sample.

Substance Mass (g) Volume (cm3)
? 9.5 2.1

What is the unknown sample made of?

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=푛푛푛푛푛푛푉푉more accurate estimates can be made with the van der waals equationí‘ťí‘ť=푛푛푛푛푛푛푉푉â’푛푛푟푟â’푞푞푛푛2푉푉2where 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?

What happens to isotopes that are unstable?

What is the approximate vapor pressure when the gas condenses at 70 degrees celsius