For the following reaction, 4.70 grams of hydrogen gas are allowed to react with 43.0 grams of iodine . hydrogen(g) + iodine(s) hydrogen iodide(g) What is the maximum mass of hydrogen iodide that can be formed? grams What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? grams

Aqueous solutions barium chloride and potassium sulfate are combined.  1) Predict the products and write the balanced equation showing the states of each substance. 2) The barium chloride solution has a volume of 100.0 mL and contains 10.00 grams of barium chloride.  The molarity of the potassium sulfate solution is 0.574 moles/liter and has a volume of 100.0 mL. Determine the limiting reactant and the mass of each product in grams. 3) Determine how many grams of excess reactant remain. 4) Calculate the molarity of just the potassium ions after the reaction has finished.

In the reaction of 28 g NO2and 18 g H2O by the chemical equation: NO2 (g) + H2O (1) → HNO3 (1) + N0 (g) a- Balanced the reaction equation. b- Calculate the moles of given reactants. c- Calculate the moles of product, HNO3. Solve it on a sheet d- Calculate the mass of HNO3 formed in grams. e- Which of the reactants is the limiting reagent? N=14g/ mol. O = 16g/mol,H=1 gmol. wwww

Combining 0.288 mol Fe,0, with excess carbon produced 16.2 g Fe. Fe,0, +3C – 2 Fe + 3 CO What is the actual yield of iron in moles? actual yield: mol What is the theoretical yield of iron in moles? theoretical yield: mol What is the percent yield?

A pile of leaves is lit on fire, and then covered completely with a fire blanket so that the fire goes out. Identify the limiting reactant in this situation.

According to the following reaction, how many grams of ammonia will be formed upon the complete reaction of 23.1 grams of hydrogen gas with excess nitrogen gas?nitrogen (g) + hydrogen (g) ammonia (g)

For the following reaction, 62.6 grams of iron(III) oxide are allowed to react with 25.4 grams of aluminum.iron(III) oxide (s) + aluminum (s) aluminum oxide (s) + iron (s)What is the maximum amount of aluminum oxide that can be formed?  grams What is the FORMULA for the limiting reagent?   What amount of the excess reagent remains after the reaction is complete?  grams

Consider the following data gathered in the "Molar Mass of a Gas" experiment.   * Mass of the empty reaction test tube: _____27.54_____ g * Mass of the test tube and MnO2 used in the reaction: ____28.04___ g * Mass of the test tube, KClO3 (MM = 122.55 g/mol) and MnO2 used in the reaction: ____29.31___ g * Mass of the test tube and its contents after the reaction: ____ (2.87x10^1) _____ g * Volume of the bubble of oxygen generated in the experiment: ___356___ mL * Atmospheric pressure in the lab: ______766.06______ mm Hg * Vapor pressure at reaction temperature: _____18.6_____ m Hg   Calculate the mass of oxygen generated in the reaction

Stoichiometry Review 1. Ammonium sulfate is used as a source of nitrogen in some fertilizers. It reacts with sodium hydroxide to produce sodium sulfate, water and ammonia, NH3. What mass of sodium hydroxide is required to react completely with 15.4 g of ammonium sulfate? 2. Iron (III) oxide, rust, can be removed from iron by reacting it with hydrochloric acid, HCl, to produce iron (III) chloride and water. What mass of hydrogen chloride is required to react with 100 of rust? 3. Dinitrogen pentoxide is a white solid. When heated it decomposes to produce nitrogen dioxide and oxygen. How many grams of oxygen gas will be produced in this reaction when 2.34 g of NO2 are made?

For the following reaction, 5.68 grams of chlorine gas are mixed with excess phosphorus (P4) . The reaction yields 5.34 grams of phosphorus trichloride .phosphorus (P4) ( s ) + chlorine ( g ) phosphorus trichloride ( l ) What is the theoretical yield of phosphorus trichloride ? grams What is the percent yield for this reaction ? %