following equation for the following: Mg3N2 + H2O → Mg(OH)2 + NH3 a. Balance the equation. b. How many moles of NH3 are produced when 0.0425 moles of Mg3N2 are reacted? c. How many grams of H₂O are needed to form 6.31 x 10-5 moles of Mg(OH)2 ? d. How many molecules of H₂O are needed to react with 0.525 lbs Mg3N2? e. How many kilograms of Mg(OH)2 are produced when 7.23 x 1027 molecules of NH3 are also produced? ithas blow asloin vier W Bra f. How many grams of Mg3N2 are needed to make 4.18 lb Mg(OH)2 ?

How many moles of iron (Fe) will be produced from 6.20 moles of carbon monoxide (CO) reacting with excess iron (III) oxide (Fe₂O 23)? Fe₂O3 + 3C0→2Fe +3CO₂ A 4.13 mol Fe 00 B C 28.01 mol Fe 3.14 mol Fe 2.68 mol Fe

Lithium used as CO2 scrubbers in spacecraft. 2(g) 315) 2 LIOH + CO à LICO + H₂O If you have 655 grams of lithium hydroxide: 1. What is the actual mole ratio? 2. What is the actual gram ratio? 3. What mass of CO, can 655 g LiOH absorb? 4. What mass of HO will be available for use? 5. What are some possible uses for the H₂O? 6. What mass of Li,CO, will be generated? 7. What will be done with the Li CO ? 8. Does it follow the Law of Conservation of Mass?

2 KMN0, + 16 HCi → 2 KCI + 2 MnCl, + 8 H,0+ 5 Cl, a. How many grams of KMN0, are needed to produce with 1.2 moles of KCl? b. How many many moles of Cl, are produced from 3.1 grams of HCl?

Given the following decomposition reaction: 4C3H5O9N3  → O2 + 12CO2 + 10H2O +6N2. a. If 28.40 g H2O were produced, what mass of CO2 will be produced?  b. If 110.5 g of C3H5O9N3 were decomposed and the yield of the reaction is 72.3%, determine the theoretical yield and actual yield.

a. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.642 mol of the first reactant were to react completely. CO₂(g) + 4H₂(g) → CH4 (9) + 2H₂O(1) mol CH4 mol H₂O b. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.622 mol of the first reactant were to react completely. BaCl₂ (aq) + 2AgNO3(aq) → 2AgCl(s) + Ba(NO3)2 (aq) mol AgCl mol Ba(NO3)2 c. For the following balanced chemical equation, calculate how many moles of products would be produced if 0.618 mol of the first reactant were to react completely. C3H8 (g) + 5O2(g) → 4H₂O(1) + 3CO₂ (9) mol H₂O mol CO₂

3. Consider the following balanced reaction: 2 Fe + 3 Cl₂ → 2 FeCl3 Given 60.0 g of Fe and excess Cl₂ (as much as we need), calculate: a. The theoretical yield of FeCl3, in grams. b. The theoretical amount of Cl₂ consumed, in grams.

a. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.255 mol of the first reactant. AgNO3(aq) + LiOH(aq) → AgOH(s) + LiNO3(aq) g AgOH g LINO3 b. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.155 mol of the first reactant. Al2(SO4)3(aq) + 3CaCl₂ (aq) → 2AlCl3 (aq) + 3CaSO4 (8) g AICI, g CaSO4 c. For the following balanced chemical equation, calculate how many grams of the products would be produced by complete reaction of 0.215 mol of the first reactant. CaCO3 (8) + 2HCl(aq) → CaCl2 (aq) + CO2(g) + H₂O(l) g CaCl2 g CO2 g H₂O Submit Answer Retry Entire Group Show Hint 9 more group attempts remaining Previous Next > Save and Exit