If 3 molecules of N, react with 6 molecules of H,, determine the number of molecules of NH, that could form from each starting material. molecules NH, 3 molecules N, x molecules NH, 6 molecules H, x Answer Bank 2 molecules NH, 1 molecule N, 3 molecules H, Determine the limiting reactant.

For each of the following unbalanced equations, calculate how many grams of each product would be produced by complete reaction of  g of the reactant indicated in boldface. Indicate clearly the mole ratio used for the conversion. ‍‍‍‍TiBr₄(g)+H₂(g)→Ti(s)+HBr(g) ‍‍‍‍‍SiH₄(g)+NH₃(g)→Si₃N₄(s)+H₂(g) ‍‍‍‍‍‍NO(g)+H₂(g)→N₂(g)+2H₂O(℩) ‍‍‍‍Cu₂S(s)→Cu(s)+S(g)

A student runs the reaction represented by the equation below. What mass of H2 gas would be produced if the student begins with 5.63 grams of each reactant? Round to the nearest 0.01 and remember to include both units and substance in your answer!!! Zn + HCl --> ZnCl2 + H2

ded for this question. When iron(III) oxide reacts with aluminum, aluminum oxide and iron are produced. The balanced equation for this reaction is: Fe2O3 (8)+2Al(s) → Al2O3 (8) + 2Fe(8) If 4 moles of aluminum react, The reaction consumes The reaction produces moles of iron(III) oxide. moles of aluminum oxide and moles of iron.

4. A mixture of glucose and oxygen reacts in acroblc respiration. The right-hand box below shows a particle diagram of the moles of substances present after the reaction is complete. On a piece of paper draw the "Before" box as shown and draw a particle diagram of the reactant molecules that produced the mixture shown on the right. Key = 02 = H20 = CO2 = CeH1206 %3D Before After You will need to draw a diagram to answer this question. On a piece of paper, draw the "Before" box as shown, and then draw a particle diagram of the reactant molecules that produced the mixture shown on the right.

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.

[References] TUTOR Chemical Equations: Gram/Gram Calculation Consider the reaction: SOe) + H;O(1) → H3SO;( Given an initial mass of 15.3 g SO, an excess of H50, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H7SO3 produced by the reaction.

Mercury can be isolated from its ore by the reaction: 4 HgS + 4 CaO → 4 Hg + 3 CaS + CaSO4     How many moles of CaS are produced from 2.5 mol CaO? Enter your answer in moles into the first answer field in accordance with the question statement. mol CaS                                 How many kilograms of Hg are produced along with 9.75 mol of CaSO4? Enter your answer in kilograms into the second answer field in accordance with the question statement. kg Hg

For the reaction shown, find the limiting reactant for each of the initial quantities of reactants. express all answers as chemical forumals  2Li(s)+Br2(l)→2LiBr(s) -1  molLi  ; 1  molBr2 -1.8  molLi  ; 1  molBr2  -2.2  molLi  ; 1  molBr2 -

How do i find the theoretical yield and how much water is produced?