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The limiting reactant when
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INTRODUCTORY CHEMISTRY-STD.GDE.+SOL.MAN
- Small quantities of ammonia gas can be generated in the laboratory by heating an ammonium salt with a strong base. For example, ammonium chloride reacts with sodium hydroxide according to the following balanced equation: :math>NH4Cl(s)+NaOH(s)NH3(g)+NaCl(s)+N2O(g) at mass of ammonia gas is produced if 1.39 g of ammonium chloride reacts completely?arrow_forwardNitrogen and oxygen react as follows: N2(g)+2O2(g)2NO2(g) Suppose 1.25mol of N2 and 50.0g of O2 are mixed together. a.Which one is the limiting reactant? b.What is the maximum mass in grams of NO2 that can be produced from the mixture?arrow_forwardThe simplest example of the hydrogenation of a carbon-carbon double bond is the reaction between ethene and hydrogen in the presence of nickel: CH2=CH2+H2NiCH3CH3. When 5.20g of ethene react with excess hydrogen gas, the reaction yields 4.75g of ethane. What is the percentage yield for this reaction?arrow_forward
- I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: 2CuCl2+4KICuCl+4KCl+I2 (a) How many molecules of I2 are produced? (b) What mass of I2 is produced?arrow_forwardA sample of calcium metal with a mass of 2.00g was reacted with excess oxygen. The following equation represents the reaction that took place: 2Ca(s)+O2(g)2CaO(s) The isolated product (CaO) weighed 2.26g. What was the percentage yield of the reaction?arrow_forwardSolid silicon dioxide, often called silica, reacts with hydrofluoric acid (HF) solution to produce the gas silicon tetrafluoride and water. a. Write the balanced chemical equation for the reaction. b. List three mole ratios, and explain how you would use them in stoichiometric calculations.arrow_forward
- What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li+N2Li3Narrow_forwardElectrolysis Determine the theoretical and percent yield of hydrogen gas if 36.0 g ofwater undergoes electrolysis to produce hydrogen and oxygen and 3.80 g of hydrogen is collected.arrow_forwardPotassium nitrate (KNO3) is used as a fertilizer for certaincrops. It is produced through the reaction 4KCl+4HNO3+O24KNO3+2Cl2+2H2O Calculate the minimum mass of KCl required to produce 567gKNO3 . What mass of Cl2 will be generated as well?arrow_forward
- Titanium dioxide, TiO2 , reacts with carbon and chlorineto give gaseous TiCl4 : TiO2+2C+2Cl2TiCl4+2CO The reaction of 7.39 kg titanium dioxide with excess Cand Cl2 gives 14.24 kg titanium tetrachloride. Calculatethe theoretical yield of TiCl4 (assuming complete reaction)and its percentage yield.arrow_forwardButane, C4H10 is a common fuel used for heating homes in areas not served by natural gas. The equation for its combustion is 2C4H10+13O28CO2+10H2O. All parts of this question are related to this reaction. a How many grams of butane can be burned by 1.42 moles of oxygen? b If 9.43g of oxygen is used in burning butane, how many moles of water result? c Calculate the number of grams of carbon dioxide that will be produced by burning 78.4g of butane. d How many grams of oxygen are used in a reaction that produces 43.8g of water?arrow_forwardThe first step in the Ostwald process for manufacturing nitric acid is the reaction between ammonia and oxygen described by the equation 4NH3+5O24NO+6H2O. Use this equation to answer all parts of this question. a How many moles of ammonia will react with 95.3 moles of oxygen? b How many moles of nitrogen monoxide will result from the reaction of 2.89 moles of ammonia? c If 3.35 moles of water is produced, how many moles of nitrogen monoxide will also be produced?arrow_forward
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