reaction of 50.0 g of aluminum and sufficient oxyger has dioxide? 2Al,0,(s) 4Al(s) + 302(g) Calculate the mass of Al;03 that can be produced if the a 75.0% yield. in oYvgen to produce carbon Tinerey

Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?

a piece of zn metal (25)g reacts with 100ml of a 2m hcl solution to form zncl2 and h2 gas. What mass of H2 will be produced if the limitng reagant is fully consumed? How many moles of limiting reagant remains after the reatioin?

6. Mg(OH)2+ H3N-> Mg3N2 + heat a. Balance the reaction b. What is the reaction type? C. If 0.540 g of hydronitric acid react in the presence of excess magnesium hydroxide, what is the theoretical yleld of water produced in grams? d. If 1.32 g of water is actually produced, what is the percent yield? e. What is the percent error?

1. Given the following reaction: (Balance the equation first!) CSHS + 02 --.....-> CO: + H:0 a. If you start with 14.8 g of C;Hy and 3.44 g of Oz, determine the limiting reagent b. Determine the number of moles of carbon dioxide produced c. Determine the number of grams H;O produced d. Determine the number of grams of excess reagent left 2. Given the following equation: Al:Os + Fe --......> Fes04 + Al a. If 25.4 of AlsOs is reacted with 10.2 g of Fe, determine the limiting reagent b. Determine the number of moles of Al produced c. Determine the number of grams of Fe;Os produced d. Determine the number of grams of excess reagent left over in the reaction

What was the actual amount of magnesium oxide (MgO) produced if the percent yield was 81.7% when 62.7 g of magnesium metal (Mg) reacted with an excess amount of carbon dioxide (CO,) ? 2 Mg + CO2- 2 MgO + C (Molar mass (in g/mol) of: Mg 24.3;C = 12.01;0 = 16.0)

What is the theoretical yield of iron in the reaction of Fe2O3+ 3CO---> 2Fe+ 3CO2 if 180.1 grams of each reactant is used?

How many moles of Pb(ONO3)2 are required to react comptely with 2.40 mol NaCl?

Given the following reaction and the molar masses below, what is the percent atom economy (% AE) for forming H2(g)?  Round to 3 sig figs    Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)