4HCl+O2---->2H2O+2Cl2 calculate the theoretical yield of H2O when 64 grams of HCl react with 19 grams of O2

Balance each reaction, then suppose exactly 13.3 g of each reactant is taken. Indicate which reactant is the limiting reagent. Calculate the mass of each product that is expected. (c) NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l)limiting reagent? NaOHCO2     Na2CO3 produced  g H2O produced  g

Al2O3 + 2Fe -------> Fe2O3 + 2Al   How many moles of Iron (III) oxide is produced from if 8.2 moles of Iron is used to react with aluminium oxide.

Question 25 of 97 Submit DDT was an insecticide used to prevent mosquito borne diseases. Due to the harmful effects on birds and fish, it is now banned in the US. However, other countries still use it to control mosquitos. It can be prepared by the reaction shown below. Determine the amount of DDT that can be produced and the percent yield for this reaction. 2C6H,CI + C2HOCI, – C,4H9CI, + H20 2 3 NEXT If a company in South America started with 1175 g of chlorobenzene (C6H5CI, MW 112.55 g/mol) and 538.5 g of chloral (C2HOCI3, MW 147.39 g/mol), set up the table below that represents 100% yield with the given reaction conditions. 2C6H,CI C2HOCI, C1.H,Cls H2O Before (mol) Change (mol) After (mol) O RESET 3.132 -3.132 3.654 -3.654 7.308 0. + -7.308 10.44 -10.44 MacBook Air F12 II F8 F10 F11 000 F9 20 F3 F7 F4 F5 F6 esc F2 F1 +.

DATA Record all masses to the maximum number of Run 1 Run 2 sig figs 200°C 400°C 1. Mass of beaker 81.061 27.986 2. Mass of beaker + NaHCO3 85.457 32.267 3. Initial mass of NaHCO3 4.476 4.292 Mass of beaker plus products after heating. 4. 84.3 80 30.742 5. Mass of product (actual yield) There are three theoretically possible chemical reactions that could occur during the thermal decomposition of baking soda. 1) sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g) 2) sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g) 3) sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g)

Consider the reaction 4Fe(s) +302(g) --> 2FE203(s) If you started with and consumed 4 moles of O2, how many moles of Fe2O3 would you produce?

Consider the following reaction: PCl3 + Cl2 -> PCl5. If the percent yield is 66.3%, what mass of PCl5 is actually formed when 61.3 g of Cl2 reacts with excess PCl3?

2 Mg(s) + O2(g) -> 2 MgO(s) When 1.5 g of magnesium burns, the theoretical yield of magnesium oxide is ____ g.

When 33.9 g of CH4 reacts completely with excess chlorine yielding 52.0 g of HCI, what is the percentage yield, according to CH418) + Cl2g) - CH3Clg) + HClig) 67.2 34.8 65.2 32.8 O 77.3

For the following reaction: C3H8(g) + 02 ——-> CO2(g) +H20(g) a). balance the reaction b). determine the limiting reactant from 20.0 grams of each starting reactant c). calculate the theoretical yield of CO2(g) in grams d). calculate the percent yield if the actual yield was 10.7 grams