Chemistry Chapter 12

Calculate the number of moles of Al2O3 that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al(s) + 3FeO(s) = 3Fe(s) + Al2O3(s) 0.20 mol; 0.40 mol; 0.60 mol; 0.90 mol

0.20 mol

How many liters of chlorine gas can be produced when 0.98L of HCl reacts with 18L O2 at STP? 0.98L; 0.49L; 3.9L; 2.0L

0.49 L

How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 2Al(s) + 3FeO(s) = 3Fe(s) + Al2O3(s) 1.2 mol; 0.8 mol; 1.6 mol; 2.4 mol

0.8 mol

Which conversion factor do you use first to calculate the number of grams of CO2 produced by the reaction of 50.6g of CH4 with O2? 1 mol CH4/16.0g CH4; 2 mol O2/1 mol CO2; 16.0g CH4/1 mol CO4; 44.0g CO2/2 mol CO2

1 mol CH4/ 16.0 g CH4

Which of the following statements about the reaction below is true? 22.4 L of CO2(g) are produced for every liter of C6H12O6(aq) reacted; 1 mol of water is produced for every mole of carbon dioxide produced; 6.02 *10^23 molecules of Na3C6H5O2 are produced for every mole of NaHCO3 used; 54g of water are produced for every mole of NaHCO3 produced

1 mole of water is produced for every mole of carbon dioxide produced

How many moles of H3PO4 are produced when 71.0g P4O10 reacts completely to form H3PO4? 0.063 mol; 1.00 mol; 4.00 mol; 16.0 mol

1.00 mol

How many moles of glucose can be "burned" biologically when 10.0 mol of oxygen is available? C6H12O6(s) + 6O2(g) = 6CO2(g) + 6H2O(l) 0.938 mol; 1.67 mol; 53.3 mol; 60.0 mol

1.67 mol

At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 2H2(g) + O2(g) = 2H2O(g) 1.8L; 3.6L; 2.0L; 2.4L

1.8 L

When iron rusts in air, iron(III) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction? 4Fe(s) + 3O2(g) = 2Fe2O3(s) 1.2 mol; 1.8 mol; 2.4 mol; 3.2 mol

1.8 mol

How many liters of hydrogen gas are needed to react with CS2 to produce 2.50 L of CH4 at STP? 2.50L; 5.00L; 7.50L; 10.0L

10.0 L

How many grams of calcium oxide are needed to produce 36.0g of Hg? 1.80g; 7,56g; 10.1g; 13.4g

10.1 g

Metallic copper if formed when aluminum reacts with copper(ii) sulfate. How many grams of metallic copper can be obtained when 54.0g of Al react with 319g of CuSO4? 21.2g; 127g; 162g; 381g

127 g

How many grams of chromium are needed to react with an excess of CuSO4 to produce 27.0g Cu? 14.7g; 18.0g; 33.2g; 81.5g

14.7 g

How many grams of beryllium are needed to produce 36.0g of hydrogen? (assume an excess of water) 4.00g; 36.0g; 162g; 324g

162 g

In the reaction 2CO(g) + O2(g) = 2CO2(g), what is the mole ratio of moles of oxygen used to moles of CO2 produced? 1:1; 2:1; 1:2; 2:2

1:2

Which of the following is an incorrect interpretation of the balanced equation show below? 2S(s) + 3O2(g) +2SO3(g) 2 atoms S+3 molecules O2=2 molecules SO3; 2gS+3gO2=2gSO3; 2molS+3molO2=2molSO3; 5 mol of reactants = 2 mol of products

2 g S + 3 G )2 = 2 g SO3

The equation below shows the decomposition of lead nitrate. How many grams of oxygen are produced when 11.5 g NO2 is formed? 1.00g; 2.00g; 2.88g; 32.0g

2.00 g

How many liters of NH3, at STP, will react with 5.3g O2 to form NO2 and water? 0.004L; 2.12L; 3.03L; 6.49L

2.12 L

How many liters of NH3 are needed to react completely with 30.0L of NO (at STP)? 5.0L; 20.0L; 7.5L; 120.0L

20.0 L

Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2Al(s) + 3H2SO4(aq) = Al2(SO4)3(aq) + 3H2(g) 0.001 mol; 10.0 mol; 15.0 mol; 22.5 mol

22.5 mol

How many grams of Fe2O3 are formed when 16.7g of Fe reacts completely with oxygen? 12.0g; 23.9g; 47.8g; 95.6g

23.9 g

How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum/ 0.85g; 290g; 450g; 870

290 g

If 1 egg and 1/3 cup of oil are needed for each bag of brownie mix, how many bags of brownie mix do you need it you want to use up all 3 eggs and 1 cup of oil? 1; 2; 3; 4

3

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 12 L of CS2. 3L CS2; 6L CS2; 9L CS2; 12L CS2

3 L CS2

Hydrogen gas is produced when zinc reacts with hydrochloric acid. If the actual yield of this reaction is 85%, how many grams of zinc are needed to produce 112 L of H2 at STP? 95g; 180g; 280g; 380g

380 g

What is the maximum number of grams of PH3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH3? 0.43g; 6.8g; 270g; 45g

6.8 g

How many grams of H3PO4 are produced when 10.0 moles of water react with an excess of P4O10? 1.22g; 6.7g; 147g; 653g

653 g

How many grams of carbon dioxide would be produced if 45 g of C6H12O6 completely reacted with oxygen? 1.5g; 1.8g; 11g; 66g

66 g

Calcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction CaCo3(s)= CaO(s) + CO2(g). What mass of lime can be produced from 1.5 * 10^3 kg of limestone? 8.4 * 10^5 kg; 8.4 *10^2kg; 8.4 kg; none of the above

8.4 * 10^2

Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9g Pb(NO3)2 are heated to give 5.5g of PbO? 44%; 56%; 67%; 82%

82%

In a particular reaction between copper metal and silver nitrate, 12.7 g Cu produced 38.1 g Ag. What is the percent yield of silver in this reaction? 56.7%; 77.3%; 88.2%; 176%

88.2%

Which of the following is true about the reaction shown below? C5H12(l) + 8O2(g) = 5CO2(g) + 6H2O(g) 9 moles of reactants chemically change into 11 moles of product; 9 grams of reactants chemically change into 11 grams of product; 9 liters of reactants chemically change into 11 liters of product; 9 atoms of reactants chemically change into 11 atoms of product

9 moles of reactants chemically change into 11 moles of product

When glucose reacts with oxygen, carbon dioxide and water are formed. How many liters of CO2 are produced when 126 G of glucose completely react with oxygen? 4.21L; 5.33L; 15.7L; 94.1L

94.1 L

Identify the limiting reagent and the volume of CO2, formed when 11 L CS2 reacts with 18 L O2 to produce CO2 gas and SO2 gas at STP. CS2-5.5 L CO2; O2- 6.0 L CO2; CS2- 11 L CO2; O2- 27 L CO2

O2- 27 L CO2

The amount of product formed when a reaction is carried out in the laboratory

actual yield

Which of the following would be the limiting reagent in the reaction shown below? 2H2(g) + O2(g) = 2H2)(g) 50 molecules of H2; 50 molecules of O2; neither a nor b is limiting; both a and b are considered limiting reagents

both a and b are considered limiting reagents

Which of the following is not a reason why actual yield is less than theoretical yield? impure reactants present; competing side reactions; loss of product during purification; conservation of mass

conservation of mass

What is the first step in most stoichiometry problems? add the coefficients of the reagents; convert given quantities to moles; convert given quantities to volume; convert given quantities to masses

convert given quantities to moles

The reactant that is not completely used up in a reaction

excess reagent

In a chemical reaction, the mass of the products _____ is less than the mass of the reactants; is greater than the mass of the reactants; is equal to the mass of the reactants; has no relationship to the mass of the reactants

is equal to the mass of the reactants

The reactant that determines the amount of product that can be formed in a reaction

limiting reagent

When two substances react to form products, the reactant which is used up is called the _____ determining reagent; limiting reagent; excess reagent; catalytic reagent

limiting reagent

This is conserved in every ordinary chemical reaction

mass

Which of the following are conserved in every chemical reaction? mass and molecules; moles and liters; mass and atoms; moles and molecules;

mass and atoms

What is conserved in the reaction shown below? N2(g) + 3F2(g) = 2NF3(g) atoms only; mass only; mass and atoms only; moles only

mass and atoms only

In any chemical reaction, what quantities are always preserved? the number of moles and the volumes; the number of molecules and the volumes; mass and number of atoms; mass and moles

mass and number of atoms

What is conserved in the reaction shown below? H2(g) + Cl2(g) = 2HCl (g) mass only; mass and moles only; mass and moles and molecules; mass moles molecules and volume

mass, moles, molecules, and volume

This quantity can always be used in the same way as moles when interpreting balanced equations

number of molecules

When 0.1 mol of calcium reacts with 880 g 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 440mL(440g)? only one half the volume of hydrogen would be produced; the volume of hydrogen produced would be the same; the volume of hydrogen produced would double; no hydrogen would be produced

only one half the volume of hydrogen would be produced

The ratio of the actual yield to the theoretical yield

percent yield

The calculation of quantities in chemical equations is called _____ stoichiometry; dimensional analysis; percent composition; percent yield

stoichiometry

Which of the following is true about limiting and excess reagents? the amount of product obtained is determined by the limiting reagent; a balanced equation is not necessary to determine which reactant is the limiting reagent; both reagents are left over after the reaction is complete; the reactant that has the smallest given mass is the limiting reagent

the amount of product obtained is determine by the limiting reagent

Which statement is true if 12 mol CO and 12 mole Fe2O3 are allowed to react? the limiting reagent is CO and 8.0 mol Fe will be formed; the limiting reagent is CO and 3.0 mol CO2 will be formed; the limiting reagent is Fe2O3 and 24 mol Fe will be formed; the limiting reagent is Fe2O3 and 36 mol CO2 will be formed

the limiting reagent is CO and 8.0 mol Fe will be formed

Which of the following is true about "yield"? the value of the actual yield must be given in order for the percent yield to be calculated; the theoretical yield is always the same as the actual yield; the percent yield may be different from the theoretical yield because reactions do not always go to completion; the actual yield may be different from the theoretical yield because insufficient limiting reagent was used

the value of the actual yield must be given in order for the percent yield to be calculated

The maximum amount of product that could be formed from given amounts of reactants

theoretical 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 ______ actual yield; percent yield; theoretical yield; minimun yield

theoretical yield

This is conserved only in reactions where the temperature is constant and the number of moles of gaseous reactants is the same as that of gaseous products

volume

Which type of stoichiometric calculation does not require the use of the molar mass? mass-mass; mass-volume; mass-particle; volume-volume

volume-volume