Diarsenic trioxide reacts with water to form arsenous acid (H3AsO3). a. Write a balanced equation for the reaction described above. b. Identify the reaction type (combustion, single replacement, double replacement, synthesis or decomposition) c.For the reaction of 68.8 g of diarsenic trioxidewith 18.8 g water, calculate the theoretical yield of arsenous acid. d. Identify the limiting reactant. e. Calculate how many grams of excess reactant remain at the end of the reaction: f. If 64.4g of arsenous acidare actually formed in the lab, calculate the percent yield for the reaction.

The combustion of liquid chloroethylene, C₂ H3 Cl, yields carbon dioxide, steam, and hydrogen chloride gas. a. Write a balanced equation for the reaction. (Use the lowest possible coefficients. Omit states of matter.) + b. How many moles of oxygen are required to react with 37.70 g of chloroethylene? moles of O₂ c. If 23.90 g of chloroethylene reacts with an excess of oxygen, how many grams of each product are formed? g CO₂ g H₂O g HCI

47. For each of the following unbalanced chemical equations, suppose 10.0 g of each reactant is taken. Show by calculation which reactant is the limiting reagent. Calculate the mass of each product that is expected. a. C3HS (g) + O2 (9) → CO2(9) + H20(g) b. Al(s) + Cl2 (g) → AICI3 (s) c. NaOH(s) + C02 (g) → Na2 CO3 (s) + H2O(1) d. NaHCO3 (s) + HCI(aq) → NaCl(aq) + H2 O(1) + CO2 (g)

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(1) g CaCl₂ g CO2 g H₂O ubmit Answer Retry Entire Group 9 more group attempts remaining Show Hint Previous Next

12. Iron metal can be obtained from iron(III) oxide by reaction with carbon monoxide at elevated temperature according to the following equation. Fe203 + 3CO → 2Fe + 3CO2 a. How many moles of iron can be obtained from 1 mole of iron(III) oxide? b. How many grams of Fe2O3 are necessary to make 50 g of iron by this reaction?

1. From the given reaction: Ca(No3)2 + Na3PO4 → Ca3(PO4)2 + NaNO3a. How many grams of sodium nitrate are produced from 1.25 grams of sodium phosphate? b. How many gra,s of calcium nitrate are required to produce 5.25 grams of calcium phosphate?2. Ibuprofen is a common painkiller used by many people around the globe. It has the formula C13H18O2. C13H18O2(s) + O2 (g) → CO2(g) + H2O (l) If a 275g tablet of ibuprofen is combusted, a. How much carbon dioxide is produced?b. How much water will be produce?c. How many oxygen are needed to produced 79.5g of water?

I only need help with the highlighted ones please :)

A. Enter the balanced chemical equation for the reaction of solid tin(II) oxide with aqueous hydrogen fluoride to produce aqueous tin(II) fluoride and water.  Express your answer as a chemical equation including phases.   B. Use your balanced chemical equation to calculate the number of moles of HFHF needed to react with 0.600 mole of SnOSnO. Express the number of moles to three significant figures.   C.Use the balanced chemical equation to calculate the grams of HFHF that need to react with 4.30 gg of SnF2SnF2. Express the mass in grams to three significant figures.   D. If 5.00 gg of HFHF completely reacts, what is the theoretical yield of SnF2SnF2? Express the mass in grams to three significant figures.

Rererences A few hydrogen and oxygen molecules are introduced into a container in the quantities depicted in the following drawing. The gases are then ignited by a spark, causing them to react and form H2O, H2 a. Write a balanced chemical equation for the reaction. (Use the lowest possible coefficients. Omit states of matter.) b. What is the limiting reactant? O2 H2 There is no limiting reactant. c. What is the maximum number of water molecules that can be formed in the chemical reaction? water molecules

5. A container containing 30.0 g of propane, C3H8, is burned with 75.0 g of oxygen. a. Outline the steps needed to determine the limiting reactant. b. Determine the limiting reactant. c. How much grams of oxygen (product) is produced?