Calculate the number of grams of carbon dioxide produced from complete combustion of one liter of octane by placing the conversions in the correct order. Make sure that the units of adjacent conversion factors cancel out. X X 1 LOctaneX 2171 g X Carbon Dioxide 8 mol CO2 114 g Octane 1000 mL Octane 1 mol Octane 1 mol Octane 8 mol CO2 1 mol Octane 1 L Octane 44 g CO2 1 mol Octane 1 mL Octane 0.703 g Octane 114 g Octane 1 mol CO2 0.703 g Octane 1 mL Octane

Use 1 decimal point for all atomic masses. 12.3 g of NCl3(g) are reacted with 0.605 g of H2(g) by the following reaction   NCl3(g) + 3H2(g) --> NH3(g) + 3HCl(g) What is the limiting reagent? NCl3(g) H2(g)     Based on the limiting reagent, what should the yield of NH3(g) be? g

Consider the following balanced equation. 3 Ag(s) + 4 HNO3(aq) → 3 AgNO3(aq) + NO(g) + 2 H2O(l) A student used 117.24 g of Ag and obtained 135.49 g of AgNO3, calculate the percent yield of AgNO3. Give your answer to the correct number of significant figures without unit. Molar mass of Ag: 107.87 g/mol Molar mass of HNO3: 63.01 g/mol Molar mass of AgNO3: 169.87 g/mol Molar mass of NO: 30.01 g/mol Molar mass of H2O: 18.02 g/mol

Q-g

Assume that your empty crucible weighs 15.98 g, and the crucible plus the sodium bicarbonate sample weighs 18.56 g. After the first heating, your crucible and contents weighs 17.51 g. After the second heating, your crucible and contents weighs 17.50 g. Answer the following questions based on this information.

Classify each chemical reaction.

Identify/label each chemical reaction according to the types listed in the table below by dragging the correct responses into the blanks. Chemical Reactions: 12FeCl2(s) + 3O2(g) → 8FeCl3(s) + 2Fe2O3(s) Br2(l) + C2H4(g) → BrCH2CH2Br(l) HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) CaCl2(aq) + K2SO4(aq) → CaSO4(s) + 2KCl(aq) Types of chemical reactions: redox reaction exchange acid-base condensation.  Please give Typed answer not hand written .

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18)(C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 4.2 kgkg of octane burned. ( HintHint: Begin by writing a balanced equation for the combustion reaction.)