Exam 3 part 1

What is the sum of all coefficients when the following equation is balanced, using the smallest whole number coefficients? Do not forget coefficients of "one". PtCl4+XeF2--->PtF6+ClF+Xe

a. 16

What is the total mass of products formed when 3.2 grams of CH4 is burned in air? CH4+2O2--->CO2+2H2O

a. 16 g

What mass of SrF2 can be prepared from the reaction of 10.0 g of Sr(OH)2 with excess HF? Sr(OH)2+2HF--->SrF2+2H2O

a. 16 g

How many molecules of O2 would react with 56 C2H6 molecules according to the following balanced equation? 2C2H6+7O2--->4CO2+6H2O

a. 196

What is the coefficient for HBr when the following equation is balanced with the smallest whole number coefficients? Br2+H2O -->HBr +HBrO3

a. 5

How many grams of KOH would have to be react with excess CO2 to produce 69.1 grams of K2CO3? 2KOH+CO2--->K2CO3+H2O

a. 56.1 g

Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". ZrO2+CCl4---> ZrCl4+COCl2

a. 6

What is the sum of all coefficients when the following equation is balanced, using the smallest whole number coefficients? Do not forget coefficients of "one". CS2+Cl2-->CCl4+S2Cl2

a. 6

Salicylic acid reacts with acetic anhydride to form aspirin, acetylsalicylic acid. How much aspirin can be produced from the reaction of 100. g of salicylic acid and 100. g of acetic anhydride? 2 C7H 6O3(salicylic acid)+C4H6O3(acetic anhydride)--->2 C9H8O4+H2O (aspirin)

d. 130 g

What is the sum of all coefficients when the following equation is balanced, using the smallest whole number coefficients? Do not forget coefficients of "one". Cl2O7+Ca(OH)2-->Ca(ClO4)2+H2O

d. 4

When heated lead nitrate decomposes according to the following equation. What is the coefficient for NO2 when the this equation is balanced with the smallest whole number coefficients? Pb(NO3)2--->PbO+O2+NO2

d. 4

In the sequential reactions shown below, the first reaction has an 80% yield and the second reaction has a 60% yield. A+B--->C+D C+E--->F What is the yield of F?

d. 48%

What mass of SrF2 can be prepared from the reaction of 8.05 g of Sr(OH)2 with 3.88 g of HF? Sr(OH)2+2HF--->SrF2+2H2O

d. 8.31 g

Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". P4 Cl2 PCl5

e. 15

How many moles of CaCO3 would have to be decomposed to produce 129 grams of CaO? CaCO3-->CaO+CO2

e. 2.30

What mass of silver nitrate, AgNO3, is required to prepare 800. g of 3.50% solution of AgNO3?

e. 28.0 g

A secondary step in the process to produce ultra-pure silicon is to combine silicon tetrachloride with magnesium. How many grams of Si could be produced by reacting 2.00 kg of SiCl4 with excess Mg? SiCl4 +2Mg-->Si+2MgCl2

e. 329.41g

What mass of Cu(NO3)2 can be prepared from the reaction of 3.65 grams of copper with 5.16 grams of HNO3? Cu+2HNO3--->Cu(NO3)2+H2

e. 7.68 g

Ultra-pure Si is required to produce semi-conductors. The first step in this process is combining silicon dioxide with carbon and chlorine. Choose the answer that represents the sum of all the coefficients when this equation is balanced using the smallest whole number coefficients. SiO2+C+Cl2--->CO+SiCl4

e. 8

The following statements apply to the interpretation of chemical equations. Not all of the statements are true. Which statement is false?

The equation A+2B--->3C+D implies that in any reaction involving A and B as reactants, A must be the limiting reactant.

How many grams of MnSO4 can be prepared from the reaction of 15.0 g of KMnO4 with 22.6 g of H2SO3? 2KMnO4+5H2SO3--->2MnSO4+K2SO4+2H2SO4

a. 14.3 g

Propane (C3H8) burns in oxygen to form CO2 and H2O according to the following equation. How many grams of O2 are required to burn 3.01 X10^23 propane molecules? C3H8+5O2--->3CO2+4H2O

a. 80.0 g

Balancing a chemical equation so that it obeys the law of conservation of matter requires:

a. Adjusting the coefficients in front of the formulas so there are the same number and type of atom on both sides of the equation.

If 25.0 g of each reactant were used in performing the following reaction, which would be the limiting reactant? 3PbO2+Cr2(SO4)3+K2SO4+H2O--->3PbSO4+K2Cr2O7+H2SO4

a. PbO2

How many moles of H2O will be produced from the complete combustion of 2.4 grams of CH4? CH4+2O2--->CO2+2H2O

b. 0.30

A mixture of calcium oxide, CaO, and calcium carbonate, CaCO3, that had a mass of 3.454 g was heated until all the calcium carbonate was decomposed according to the following equation. After heating, the sample had a mass of 3.102 g. Calculate the mass of CaCO3 present in the original sample. CaCO3 (solid)-->CaO (solid)+CO2 (gas)

b. 0.800 g

Suppose 600. g of P4 reacts with 1300. g of S8. How many grams of P4S10 can be produced, assuming 80.0% yield based on the limiting reactant? 4P4+5S8--->4P4S10

b. 1.44X10^3 g

Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". XeF2+H2O--->Xe+HF+O2

b. 11

The reaction of a hydrocarbon with oxygen to produce CO2 and water is called complete combustion. Write the balanced reaction for the complete combustion of heptane, C7H16, with the smallest whole number coefficients. Then choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one".

b. 27

Balance the following equation with the smallest whole number coefficients. What is the coefficient for NH3 in the balanced equation? Fe(NO3)3+NH3+H2O--> Fe(OH)3+NH4NO3

b. 3

If sufficient acid is used to react completely with 72.9 g of magnesium, how much hydrogen will be produced? 2HCl+Mg--->MgCl2+H2

b. 3.0 mol

The single largest use of phosphoric acid is in the production of fertilizer. How many grams of phosphoric acid (with excess NH3) are required to produce 800 g of (NH4)2HPO4, a common fertilizer? H3PO4+2NH3--->(NH4)2HPO4

b. 593 g

The discharge reaction that occurs in a nickel-cadmium (nicad) battery is shown below. Choose the answer that represents the sum of all the coefficients when this equation is balanced using the smallest whole number coefficients. Cd+NiO2+H2O--->Cd(OH)2+ Ni(OH)2

b. 6

If a reaction of 5.0 g of hydrogen with 5.0 g of carbon monoxide produced 4.5 g of methanol, what was the percent yield? 2H2+CO--->CH3OH

b. 79%

Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". Cr+H2SO4--->Cr2(SO4)3+ H2

b. 9

One of the reactions that take place inside a blast furnace to produce iron is the reduction of iron ore by carbon monoxide. Choose the answer that represents the sum of all the coefficients when this equation is balanced using the smallest whole number coefficients. Fe2O3+CO--->CO2+Fe

b. 9

If 20.0 g of each reactant were used in performing the following reaction, which would be the limiting reactant? 2MnO2+4KOH+O2+Cl2--->2KMnO4+2KCl+2H2O

b. KOH

What scientific law requires that subscripts in formulas should never be changed while balancing a chemical equation?

b. Law of Definite Proportions

Balance the following equation with the smallest whole number coefficients. Choose the answer that is the sum of the coefficients in the balanced equation. Do not forget coefficients of "one". CuSO4+NH3+H2O --->(NH4)2SO4+Cu(NH3)4(OH)2

c. 11

How many grams of O2 are required to burn 46.0 grams of C5H12? C5H12+8O2 --->5CO2+6H2O

c. 164 g

Ammonium nitrate fertilizer is sometimes used as an explosive. How many moles of water can be formed from the decomposition of 13.2 moles of ammonium nitrate? 2NH4NO3--->2N2+O2+4H2O

c. 26.4

How many grams of PI3 could be produced from 250. g of I2 and excess phosphorus if the reaction gives a 98.5% yield? P4+6I2--->4PI3

c. 266 g

The density of a 7.50% solution of ammonium sulfate, (NH4)2SO4, is 1.04 g/mL. What mass of (NH4)2SO4 would be required to prepare 750. mL of this solution?

c. 58.5 g

What is the percent yield if 28.50 of FeO reacts with excess CO and produces 17.841 g Fe? FeO+CO--->Fe+CO2

c. 80.55%

What is the percent yield of CO2 if the reaction of 10.0 grams of CO with excess O2 produces 12.8 grams of CO2? 2CO(g)+O2(g)--->2CO2(g)

c. 81.5%

What mass of phosphoric acid, H3PO4, would actually react with 7.17 grams of LiOH? 3LiOH+H3PO4--->Li3PO4+3H2O

c. 9.80 g

Which of the following is not a consequence of the Law of Conservation of Matter?

c. As a result, there will be the same number of moles on both the reactant and the product side of a balanced equation.

Ethyl butyrate (C6H12O2), "oil of pineapple", can be produced in the laboratory from butyric acid (C4H8O2), a foul-smelling liquid, and ethyl alcohol (C2H6O). First, butyric acid is reacted with PCl5 to produce butyryl chloride (C4H7ClO) which is then reacted with the ethyl alcohol to produce the ethyl butyrate. What mass of ethyl butyrate could be produced from 12.8 g of butyric acid if the first reaction gave a 65.8% yield of butyryl chloride and the second reaction gave a 88.4% yield of ethyl butyrate? C4H8O2+PCl5--->C4H7ClO+HCl+POCl3 C4H7ClO+C2H6O--->C6H12O2+HCl

e. 9.81 g

If 6.6 g of fluorine reacts with 5.6 g chlorine to produce 8.5 g of chlorine trifluoride, what is the limiting reactant and the percent yield of chlorine trifluoride? Cl2+3F2--->2ClF3

e. F2, 79%