Chem Lab Quiz 7, 8, 9

Front 1

Addition of HNO3 to Copper

Back 1

Causes copper metal to slowly dissolve and produce a brown gas.

Front 2

Cu(NO3)2 + NaOH

Back 2

Metathesis Reaction, solution turns bright blue. Products are Cu(OH)s + 2NaNO3 (aq)

Front 3

Washing and Decanting CuO and water

Back 3

Removes excess NaNO3 and impurities

Front 4

When you add H2SO4, what copper compound is now present?

Back 4

Copper (II) sulfate

Front 5

CuSO4 (aq) + Zn (s)

Back 5

Produces hydrogen gas, Zn2+ ions and SO4 2- ions are present in the solution. *When acid is added to a metal, hydrogen gas is produced

Front 6

Possible Sources of Error in Copper Experiment

Back 6

1. Not drying sample completely, so SO4 is still present

2. Other elements are mixed in with copper

Front 7

Percent Yield Formula

Back 7

(Actual Yield / Theoretical Yield) * 100%

Front 8

Relationship between pressure and volume of a gas at constant temperature

Back 8

As volume decreases, pressure increases

Front 9

Relationship between temperature and pressure of a gas at a constant volume

Back 9

As temperature increases, pressure increases

Front 10

Ideal Gas Law

Back 10

PV = nRT

Front 11

Accepted Value of R

Back 11

0.0821

Front 12

Number of Moles of a Substance

Back 12

Equals the mass of the substance in grams, m, divided by the molar mass, M

Front 13

Molar Mass Related to Ideal Gas Law

Back 13

PV = (m/M)RT

M = (mRT)/PV

Front 14

Van der Waals Equation

Front 15

(N^2a)/v^2

Back 15

Correction to pressure, takes into account intermolecular attractions

Front 16

Nb

Back 16

Correction for the finite volume of the molecules

Front 17

Atmospheric Pressure

Back 17

Pressure of O2 + Pressure H2O vapor

Front 18

Purpose of Equalizing Clamp

Back 18

To produce atmospheric pressure inside the bottle and test tube

Front 19

Opening pinch clamp

Back 19

Water flows into beaker. If the system remains airtight and has no leaks, tube A will remain filled with water

Front 20

Volume of water displaced

Back 20

Equal to volume of oxygen produced

Front 21

Difference in mass between the tube plus the contents and the original mass of the tube plus MnO2 and KClO3

Back 21

Mass of oxygen produced

Front 22

a for O2

Back 22

1.360

Front 23

a for O2

Back 23

1.360

Front 24

b for O2

Back 24

31.83

Front 25

Cause for derivation from ideal gas behavior

Back 25

Attractive forces between molecules

Front 26

If an insufficient amount of liquid unknown had been used, how would the value of the experimental molar mass been affected?

Back 26

The liquid wouldn't occupy the whole container and the volume in the formula would be greater than it actually is and there would be a smaller molar mass

Front 27

Major sources of error in determining molar mass

Back 27

Too big hole in aluminum, inaccurate temp reading, inaccurate volume measured, inaccurate weight measured