20 POINTS When methane, CH4, is combusted, and produces carbon dioxide, CO2, according to the unbalanced equation CH4 +02 —>CO2 + H2O Write the balanced equation for this reaction, and explain how it is possible for 10 grams of methane fuel to burn in and emit 27 grams of carbon dioxide. Discuss whether or not this reaction obeys the law of conservation of mass.

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?

Calculate the molarity of 48.0 ml of 6.00 m h2so4 diluted to 0.250 l .

How many moles of sulfur dioxide are produced when 4.38 moles of oxygen completely react with iron (iv) sulfide