Go to the molecules mode by selecting the icon at the bottom. notice that there are three real reactions: the synthesis of water, the synthesis of ammonia, and the combustion of methane. select each of the reactions and observe the reactants taking part in the reactions. suppose you are carrying out each of these reactions starting with five moles of each reactant. observe that some reactants are in excess whereas some reactants limit the amount of products formed. classify each of the reactants as a limiting reactant or an excess reactant for a reaction starting with five moles of each reactant. drag the appropriate items to their respective bins.

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?

According to the tide table below what time of day will the highest tide occur?

What term describes technology that operates on an atomic level