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Using the reaction below write out a complete setup for the following stoichiometry on a sheet of paper. Make sure to have complete conversion factors with units in the correct order of calculation and sig figs for final answer. Upload as a pdf file or write in text box. C4H8(g) + 6 O2(g) 4 CO2(g) + 4 H20(g) How many liters of carbon dioxide gas can be created if I start with 45.63 grams of oxygen gas?

Reactants Products Before reaction 3 mol N, 6 mol H, O mol NH, After reaction 1 mol N2 O mol H2 4 mol NH, Reaction in presence of limiting reagent. Ammonia, NH3, is created from the reactants N2 (shown in green) and H2 (shown in white) according to the following balanced chemical equation. In the example above you begin with 3 mol of nitrogen gas and 6 mol of hydrogen gas. N2+3H2----> 2NH3 Which is the limiting reactant? You can tell that hydrogen is the limiting reactant because all of it was used up, but there is some leftover (excess) nitrogen in the diagram when the reaction is complete Since the mole ratios match up perfectly between the reactants neither of them is limiting. You can tell that ammonium is the limiting reactant because there were 0 moles of it before the reaction started. You can tell that nitrogen gas is the limiting reactant because there were fewer moles of it with which to begin.

Please refer to the image i need this done asap pleaseeee show the work