Chemistry 1111 Final Exam Review

Front 1

A yellow flame indicates too _____ oxygen.

Back 1

Little

Front 2

You make the following measurement on a metal cylinder: d=1.25 cm; l=3.61 cm. The mass of the cylinder is 7.42g. Calculate the density.

Back 2

(7.42g)

__________________________=4.43cm^3

(Pi ((1.25cm/2)^2)3.61cm)

Front 3

How did you determine the volume of the glass beads?

Back 3

Geometric Measurement and Volume Displacement

Front 4

What is specific heat?

Back 4

amount of heat necessary to raise the temperature of one gram of a substance by one degree celcius.

Front 5

Suppose you heat 6.3g of an unknown metal block to 100 degrees celcius and then drop the metal into a calorimeter containing 50.0g of H2O at 19.0 degrees celcius. Assume that there is no heat lost to the calorimeter. The final temperature of the water in the calorimeter and the metal bloack is 26.6 degrees celcius. Calculate the specific heat of the metal.

Back 5

[-(50.0g)(4.18J/gs)(26C*-19C*)]

_______________________________ =3.443J/gc

[(6.3g)26.6C*-100C*)]

Front 6

Mg metal is added to a solution of hydrochloric acid. Colorless bubbles are given off. Write a balanced molecular equation and convert it a net ionic equation.

Back 6

Mf(s) + 2HCl2(aq)>>>> MgCl2(aq)+H2(g)

Mg(s)+H(aq)>>>>Mg2(aq)+H2(g)

Front 7

Write down the copper cycle

Back 7

Cu(s){bronze}>>>>Cu(NO3)2(aq){green}>>>>Cu(OH)2(s){blue}>>>>Cu(s){black}>>>>CuSO4(aq){blue}

Front 8

Which products in the pathway are solids and which are solutions?

Back 8

Solids: (Cu,Cu(OH)2, CuO)

Solutions: (Cu(NO3)2, CuSO4)

Front 9

What reagents are needed to go from step to step?

Back 9

Nitric acid, Sodium Hydroxide, Heat, Sulfric Acid, and water, Zinc and HCl

Front 10

What poisonous gas was generated in the cycle?

Back 10

NO2 aka nitrogen oxide in step one

Front 11

How much copper is contained in 100g of CuO

Back 11

100g CuO X (63.546gCu)

______________ =79.9g of Cu

(79.545gCuO)

Front 12

What is the principal reaction?

Back 12

2Mg(s)+O2>>>>MgO(s)

Front 13

Were there any other products formed other than MgO?

Back 13

Mg3N2

Mg(OH)2

H2O

Front 14

Calculate the % Mg given the following data: weight of crucible, cover and lid=30.15g; weight of crucible, cover, lid and Mg=32.19g; weight of crucible, cover, lid and oxide=33.76g

Back 14

32.19-30.15=2.04gMg

33.76-30.15=3.61gMgO

(2.04/3.61) X 100=56.5%

Front 15

A mixture contains 15.0g KClO3 and 20.3g NaCl. What is the % KClO3 (by weight)?

Back 15

(15.0/35.3) X 100=42.49% KlCO3

Front 16

What is the reaction that describes the decomposition of KClO3?

Back 16

2KClO3>>>>2KCl+3O2

Front 17

How much O2 will be generated in mols beginning with 0.107mol KClO3?

Back 17

0.160 mol )2 X 32g)2/ 1mol)2 = 5.14gO2

Front 18

What is a hydrate?

Back 18

A compound that integrates intact H2 molecules into its crystal structure

Front 19

Suppose you obtain 0.0166 mol for the amount of anhydrous salt and 0.1328mol for the amount of water. What is the formula of the hydrate (x)?

Back 19

(0.1328mol)/(0.0166mol)=8H2O

Front 20

How many liters of 12.0M H2SO4 (aq) would it take to supply 0.155mol of H2SO4?

Back 20

12.0M/0.155mol=0.012916 L

Front 21

The vapor pressure of water at 20.0C* is 17.5 torr. Suppose you collect 500 ml of an unknown gas over the water at 25.0C*, how many mols of has are ther in the flask? The barometric pressure is 760mmHg.

Back 21

n=(0.977 atm)(0.5L)/(0.0821)(293)=0.0203mol

Front 22

Suppose a photon has an energy of 1.8 X 10^-19 J. What is its correspoinding frequency?

Back 22

V= 6.626 X 10^-34J-1.8 X 10^-19J=-1.8 X 10^-19