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chem ch 12 test
Terms in this set (33)
if one knows the mass and molar mass of reactant A and the molar mass of product D in a chemical reaction, one can determine the mass of product D produced by using the
mole ratios of D to A from the chemical equation
actual yield must be determined by
to determine the limiting reactant in a chemical reaction involving known masses of the two reactants, A and B, which of the following calculations would be the most useful?
calculating the mass of a single product formed from each reactant
metallic copper is formed when aluminum reacts with copper(II) sulfate. how many grams of metallic copper can be obtained when 54.0 g of Al react with 319g of CuSO4?
what is the measured amount of a product obtained from a chemical reaction?
what is needed to calculate the mass of ammonia gas produced from 2.0 L of nitrogen gas in excess hydrogen gas in the reaction below? N2(g)+3H2(g)->2NH3(g)
two molar masses, one density, and one mole ratio
to determine the limiting reactant in a chemical reaction, one must know the
avaliable amount of each reactant
a balanced chemical equation allows one to determine the
mole ratio of any two substances in the reaction
which of the following would be the limiting reagent in the reaction shown below? 2H2(g)+O2(g)->2H2O(g)
50 molecules of O2
the actual yield of a chemical reaction is
less than the theoritical yield
when an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called the
what is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
which of the following statements about the reaction below is true? 3NaHCO3(aq)+C6H8O7(aq)->3CO3(g)+Na3C6H5O7(aq)
1 mole of water is produced for every mole of carbon dioxide produced
the substance not completely used up in a chemical reaction is known as the
which of the following is true about "yield"?
the actual girld may br different from the theoretical yield because insufficient limiting reagent was used
which statement is true if 12mol CO and 12 mol Fe2O3 are allowed to react?
the limiting reagent is CO and 8.0 mol Fe will be formed
methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. identify the excess reagent and calculate how much remains after 36L of H2 reacts with 12L of CS2? 4H2(g)+CS2(g)->CH4(g)+2H2S(g)
the substance that restricts the participation of other reactants in a chemical reaction is known as the
calcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction CaCO2(s)->CaO(s)+CO2(g). what mass of lime can be produced from 1.5*10^3 kg of limestone?
what is the maximum number of grams of PH2 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH3? P4(g)+6H2(g)->4PH3(g)
the coefficients in a chemical equation represent the
relative numbers of moles of reactants and products
identify the limiting reagent and the volume of CO2 formed when 11L CS2 reacts with 18L O2 to produce CO2 gas and SO2 gas at STP? CS2(g)+3O2(g)->CO2(g)+2SO2(g)
O2; 6.0 L CO2
a chemical reaction involving substances A and B steps when B is completely used. B is the
in the reaction, CH4(g)+2O2(g)+2H2O(g), a mass of 25g CO2 is produced by reacting methane with excess oxygen. the following expression calculates the
moles of methane consumed
when 0.1 mol of calcium reacts with 880g of water, 2.24 L of hydrogen gas form (at STP). how would the amount of hydrogen produced change if the volume of water was decreased to 440 mL (440g)?
the volume of hydrogen produced would be the same
when two substances react to form products, the reactant which is used up is called the
in the chemical equation wA+xB->yC+zD, a comparison of the number of moles of A to the number of moles of C would be a
which of the following is true about limiting and excess reagents?
the amount of product obtained is determined by the limiting reagent
in the chemical equation wA+xB->yC+zD, if one knows the mass of A and the molar masses of A, B, C, and D, one can determine
the mass of any of the reactants or products
which of the following is NOT a reason why actual yield is less than theoretical yield?
conservation of mass
hydrogen gas is produced when zinc reacts with hydrochloric acid. of the actual yield of this reaction is 85%, how many grams of zinc are needed to produce 112 L of H2 at STP? Zn(s)+2HCl(aq)->ZnCl2(s)+H2(g)
how many mole ratios can be correctly obtained from the chemical equation 2NO->N2+O2?
in the chemical equation wA+xB->yC+zD, how many correct mole ratios can be obtained that relate only the products?
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