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For each of the following reactions, calculate the grams of indicated product when 15.0 g of the first reactant and 10.0 g of the second reactant are used:
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- 4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) identify the limiting reactant, and explain how the pictures allow you to do so.arrow_forwardFollow the rules of significant digits. Balance the reaction below. How many moles of oxygen gas reacted if 5.32 moles of carbon dioxide were produced? C3H16 (g) + 02 (g) --> CO2 (g) + H20 (g)arrow_forwardUse the following reaction to answer the question that follow: Fe,O3 (s) + 3CO J 2Fes + 3CO a) Determine the limiting reactant when 80.0 grams of Fe,O3 (Molar Mass = 160 g/mol) are reacted with 36.0 grams of CO (Molar Mass = 28.0 g/mol) %3D %3Darrow_forward
- Propane combusts via the following unbalanced reaction: C3H8+O2→H2O+CO2 When 36.15 g of propane is combusted in excess oxygen, how many grams of CO2 are produced and how many grams of O2 are consumed?arrow_forwardConsider the following balanced equation for the combustion of propane: C3H3 (g) + 502 (g) → 3CO2 (g) + 4H,0 (g) 10) If 10.0 g of propane are mixed with 10.0 g of oxygen, (a) How many moles of each reactant are mixed? (3 significant figures) C3Hg: O2:arrow_forwardHydrogen gas can be produced by the reaction of magnesium metal with hydrochloricacid according to the following equation:Mg(s) + 2HCl(aq) > MgCl2(aq) + H2(g)How many grams of Magnesium chloride are formed when 6.00 grams of HCl reactswith 5.00 grams of Mg? (Answer to one decimal place)grams of Magnesium chlorideWhat is the limiting reactant? HCI or Mg? Show all workarrow_forward
- Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is:2Mg(s)+O2(g)→2MgO(s)2Mg(s)+O2(g)→2MgO(s) When 10.1 gg of MgMg are allowed to react with 10.5 gg of O2O2, 11.7 gg of MgOMgO are collected. Determine the theoretical yield and the percent yield for the reaction.arrow_forward2NO(g) + O2(g) → 2NO2(g) You are provided with 4.12 molmol of nitrogen monoxide gas. Using the balanced chemical equation completed in Part A, determine how many moles of oxygen gas are needed to completely react with the nitrogen monoxide gas and how many moles of nitrogen dioxide are formed as a result? Ammonia and oxygen react to form nitrogen monoxide and water. Construct your own balanced equation to determine the amount of NO and H2O that would form when 2.80 molmol NH3 and 4.64 mol O2 react. Express the amounts in moles to two decimal places separated by a comma.arrow_forward18: 4 Al (S) + 302(g) 2AI2O3(s) When 47.90 g of Al and 80.13 g of O, were reacted, 14.22 grams of aluminum oxide were obtained. What is the percent yield? (Hint: You need to determine which one is the limiting reactant and then the theoretical yield). 9: Your Answer: CO: Answer unitsarrow_forward
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