Consider the unbalanced equation for the combustion of hexane: αC6H14(g)+βO2(g)→γCO2(g)+δH2O(g) Determine how many moles of O2 are required to react completely with 7.4 mol of C6H14.   Express your answer using two significant figures.

The balanced equation for the decomposition of potassium chlorate is shown below. When carried out in lab, this reaction is found to produce 1.2 g of potassium chloride. For your convenience, the molar mass of each substance Is shown below their formulas (in purple). Use this Information to make the requested calculation: 2 KCIO3(s) -> 2 KCI(s) + 3 02(g) 122.551 74.551 32 Determine the percent yield if the reaction consumes 2900 mg of potassium chlorate:

2NO(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.

Honors Chemistry Chapter 9 Name/Date 3. Gold is very valuable because it does not oxidize easily. It can be oxidized by reacting it with nitric acid as shown below: Au(s) + 4H'(aq) + NO: (aq) → NO(g) + 2H:0(g) + Au³ (aq) 3a. If 30 grams of gold react with 3.4 grams of nitrate ion, which reactant is limiting?. 3b. What is the theoretical yield?. 4. Lead (II) nitrate reacts with sodium chloride according to the equation below: Pb(NO.): + NaCl → PbCla + NANO. 4a. If 8.3 grams of lead (II) nitrate react with 5 grams of sodium chloride, which material would be the limiting reactant? 4b. What is the theoretical yield?

For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 9 moles of methane, CH4 ?

The balanced equation for the combustion of butane, CaH1o, is shown below. For your convenience, the molar mass of each substance is shown below their formulas (in purple). Use this information to make the requested calculation: 2 CAH10(g) + 13 02(g) -> 8 CO2(g) + 10 H20(1) 58.124 32 44.011 18.016 What mass of butane, in kg, will be needed to react fully with 250 L of oxygen gas?

Consider the reaction: C2H4 + O2     →     CO) (Unbalanced).  If 0.96 g of C2H4 g was Used 5.2 g of CO2 produced, calculate the percentage yield in the reaction. (Hint Balance the equation first).

What mass of CO2 (in Kg) does the combustion of a 12-gallon tank of gasoline release into the atmosphere? Assume the gasoline is pure octane (C8H18) and that it has density of 0.70 g/mL. You will need a balanced chemical equation for combustion of octane.

Consider the following unbalanced chemical equation: Fe3O4 (aq) + CO (g) → CO2 (g) + Fe (s) What will be the coefficient in front of CO in the balanced chemical equation? If there is no coefficient in front of CO in the balanced equation, enter 1 as the answer.

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.