Percent comp and atomic mass(1)

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▼ Part A Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li (s) + N₂ (g) → 2Li3N (s) How many moles of lithium are needed to produce 0.27 mol of Li-N when the reaction is carried out in the presence of excess nitrogen? O 1.6 O 0.81 O 0.14 O 0.090 O 0.18 Submit 4 Request Answer

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Question 15 You determined the theoretical yield for Znl2 if 0.5 moles of zinc is used to form Znl2. Determine the percent yield if 189.6 g of Znl, product is recovered. Zn + _12 → Znl2 0 87% 0 94.9% 93.7% 0 97%

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Stoichiometry Knowledge check 4.Given the balanced chemical equation below, determine the mass of CaCl2 produced if 4.9 g of Ca(OH)2 reacts with 18 g of HCl. Ca(OH)2 + 2HCl --> CaCl2 + 2HOH   g CaCl2 How many grams of excess reactant remains after the reaction occurs?   g   Blank 1:  Blank 2:

Review - A Bookmark Mole Concept S21 / 1 of 16 In the balanced chemical reaction shown below, what is the mole ratio between Fe and Al? Fe2O3(s) + 2AI(s) 2Fe(s) +Al2O3(s) ОА. 1 to 1 Ов. 1 to 2 С. 2 to 1 O D. 3 to 1

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I Review I Constants I Periodic Table Learning Goal: Consider a situation in which 235 g of P4 are exposed to 272 g of O2 . To calculate theoretical and percent yields, given the masses of multiple reactants. A balanced chemical reaction gives the mole ratios between reactants and products. For example, one mole of white phosphorus, P4, reacts with five moles of oxygen, O2 , to produce two moles of diphosphorus pentoxide, P205 : Part A What is the maximum number of moles of P2O5 that can theoretically be made from 235 g of P4 and excess oxygen? Express your answer to three significant figures and include the appropriate units. P4 + 502→2P2O5 In this example, if we know the number of moles of phosphorus, we know that twice that much product can be made, assuming we have enough oxygen. Similarly, if we know the number of moles of oxygen, we know that two-fifths that much product can be made, assuming we have enough phosphorus. In a situation where you are given the mole amounts of both…

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What amount of carbon dioxide (in moles) is produced by the reaction of 5.00 mol CH12 with 30.0 mol 0,? C;H12(g) + 8 O2(g)5 CO2(g) + 6 H,O(g) O 48.0 mol O 25.0 mol O 3.13 mol O 18.8 mol O 150 mol Submit Answer Try Another Verslon 1 item attempt remaining

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2nd question using the train track method

Stoichiometry Knowledge check 5.A student obtained 11.1 g of Al2S3 from the following reaction. The student added 19.5 g of Sodium sulfide to 19.5 g of Aluminum phosphate. 3Na2S + 2AlPO4 --> 2Na3PO4 + Al2S3 What is the percent yield of Al2S3 from the reaction listed above?   %

Macmillan Learning The reaction for producing glucose in plants, called photosynthesis, is light 6CO₂ +6H₂0- + C6H₁206 +60₂ If a plant produces 8.41 mol CH₁2O6, how many moles of H₂O are needed? moles H₂O: x10 TOOLS mol

Stoichiometry Knowledge check 2.Given the following balanced chemical equation, how many grams of HOH would be produced when 34.78g of Iron (III) hydroxide is mixed with an excess amount of sulfuric acid? 2Fe(OH)3 + 3H2SO4 --> 6HOH + Fe2(SO4)3  ______g HOH All work must be shown and submitted. Any steps left out may result in a loss of points for that particular problem.

A sample of dichlorodibromosilane, SiCl₂Br2, contains 0.0402 mol of the compound. What is the mass of the sample, in grams? 9 Submit Show Approach Show Tutor Steps

Practice Indicate the limiting reactant shown in the following illustration: Zn(s) + S(s) ZnS(s) Zn S

How many moles of H2SO, are required to completely react with 7.20 mol of AlI according to the balanced chemical reaction: 2 Al(s) + 3 H2SO,(aq) → Alz(SO4)3(aq) + 3 H2(g) STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 342.14 3 7.20 2 26.98 98.08 21.6 3.60 10.8 2.02 6.022 x 1023 2.40 mol Al g H2 g Al mol Al2(SO4)3 mol H2SO4 mol H2 g Al2(SO4)3 g H2SO,