Chemistry

Question 1

E - 2, LP - 0

Answer 1

Linear

Question 2

E - 3, LP - 0

Answer 2

Trigonal Planar

Question 3

E - 3, LP - 1

Answer 3

Bent

Question 4

E - 4, LP - 0

Answer 4

Tetrahedral

Question 5

E 4 LP 1

Answer 5

Trigonal Pyramid

Question 6

E 4 LP 2

Answer 6

Bent

Question 7

E 5 LP 0

Answer 7

Trigonal Bipyramidal

Question 8

E 5 LP 1

Answer 8

See Saw

Question 9

E 5 LP 2

Answer 9

T Shape

Question 10

E 5 LP 3

Answer 10

Linear

Question 11

E 6 LP 0

Answer 11

Octahedral

Question 12

E 6 LP 1

Answer 12

Square Pyramidal

Question 13

E 6 LP 2

Answer 13

Square Planar

Question 14

Linear Charge

Answer 14

Non Polar

Question 15

Trigonal Planar Charge

Answer 15

Non Polar

Question 16

Bent Charge

Answer 16

Polar

Question 17

Tetrahedral Charge

Answer 17

Non Polar

Question 18

Trigonal Pyramid Charge

Answer 18

Polar

Question 19

Trigonal Bipyramidal Charge

Answer 19

Non Polar

Question 20

See Saw Charge

Answer 20

Polar

Question 21

T Shape Charge

Answer 21

Polar

Question 22

Octahedral Charge

Answer 22

Non Polar

Question 23

Square Pyramid Charge

Answer 23

Polar

Question 24

Square Planar Charge

Answer 24

Non Polar

Question 25

If a molecule is polar it has what forces?

Answer 25

Dipole Dipole

Question 26

Higher Temperatures do what to vaporization pressure

Answer 26

Increase

Question 27

Higher Surface Areas do what to vaporization pressure?

Answer 27

Increase

Question 28

Container Size does what to vaporization pressure?

Answer 28

Increase

Question 29

Weaker Intermelecular forces do what to vaporation pressure

Answer 29

Higher Vaporization pressure. Water has Hydrogen bonding and will vaporize slower than compounds with weaker intermolecular forces

Question 30

Equation to get Molarity (M)

Answer 30

amount of solute (In mol) / volume of solution (In L)

Question 31

Equation to get Molality (m)

Answer 31

Amount of solute (in mol) / mass of solvent (In kg)

Question 32

Equation of mole fraction (x)

Answer 32

amount of solute (in mol) / total amount of solute and solvent (in mol)

Question 33

Equation for Mole Percent (mol %)

Answer 33

amount of solute (in mol) / total amount of solute and solvent (in mol) x100%

Question 34

Equation of parts by volume (%, ppm, ppb)

Answer 34

volume solute / volume solution x multiplication factor

Question 35

What is c?

Answer 35

Specific Heat

Question 36

How much heat in kJ is required to convert 55.0 g benzene at –15.5 ˚C to benzene at 42.4 ˚C? How do you do this problem.

Answer 36

You find the molar mass of the compound. Find how many rate changes there are. q=mcat for the first phase (IN J) mass->molar mass->enthalpy (given) (IN KJ) q=mcat for last phase (IN J) Convert to KJ Add together

Question 37

At 20°C, an aqueous solution that is 20.0% ammonium chloride by mass has a density of What is the molarity of ammonium chloride in the solution? The formula weight of Cl is How do you solve this problem.

Answer 37

Its asking for the molarity so you use the molarity formula which is amount of solution (in mol) / volume of solution (in L) you start by assuming 100g of solution. convert 100g->given g/ml->1000mL in a L this calculation gives you the L Then you take the assumed amount of solute (20g) and convert it with the mol value you were given. plug in with the molarity formula

Question 38

At 20°C, a 1.33 M aqueous solution of ammonium chloride has a density of What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is How do you solve this problem?

Answer 38

You are wanting to find the molality which is amount of solute (in mol) / mass of solvent (in kg) you are given the Moles of the solution and need to assume 1L 1L-1000mL->given amount for mL then you take the Moles you were given 1.33->amount given for mol then divide these numbers amount of solute (in mol) / mass of solvent (in kg)

Question 39

Is the solute or solvent usually in a lower amount?

Answer 39

Solute

Question 40

At 20°C, a 0.756 M aqueous solution of ammonium chloride has a density of What is the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is How do you solve this problem?

Answer 40

It is asking for the mass percent which is amount of solute (in g) / total amount of solution (in g) you can assume 1 L->1000mL->given amount of mL then you take the moles given 0.756->given amount of mols in g solute/total x 100

Question 41

what is the equation for vapor pressure

Answer 41

Psoln = (xSolvent)(PSolvent)

Question 42

what does P mean?

Answer 42

Vapor Pressure

Question 43

A solution is prepared by adding 20.00 g of lactose (milk sugar) to 110.0 g of water at The partial pressure of water above the solution is ________ torr. The vapor pressure of pure water at 55°C is 118.0 torr. The molar mass of lactose is How do you solve this problem.

Answer 43

Whenever you see vapor pressure you need to use the equation psoln = (xSolvent)(PSolvent) the PSolvent will most likely be given Using what you are given which in this case is the mass in grams of the substances, convert both to moles take the moles of solvent / total moles take that number and multiply it by the vapor pressure of the solvent the solvent is the higher amount

Question 44

A solution is prepared by dissolving 5.00 g of glycerin ( ) in 201 g of ethanol The freezing point of the solution is ________°C. The freezing point of pure ethanol is at 1 atm. The molal-freezing-point-depression constant ( ) for ethanol is The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively How do you solve this problem?

Answer 44

When you see the freezing point, you use the equation DeltaTf = (m)(kf) to get the molality you use the equation moles of solute / kg of solvent take the given grams of the solute and convert to moles convert the given grams of solvent to kg divide multiply by the given kf take the freezing point and subtract the value you calculated

Question 45

What is the expected freezing point of a 0.50 m solution of Na2SO4 in water? Kf for water is 1.86°C/m. how do you solve this?

Answer 45

It might look like you have all of the information to do the simple problem but you have to factor in the van hoff factor (i) mutiply everything by 3

Question 46

The reaction is first order and has a rate constant of 4.82 × at 64°C. If the reaction is initiated with 0.092 mol in a 1.00-L vessel, how many moles remain after 151 s How do you solve this?

Answer 46

If you see "Initiated" you are using the equation ln[A]t = -kt+ln[A]0 plug in all the numbers and then take that number and remember do e^the calculated number

Question 47

What is k?

Answer 47

Rate Constant

Question 48

For a particular first-order reaction, it takes 6.0 minutes for the concentration of the reactant to decrease to 25% of its initial value. What is the value for rate constant (in s-1) for the reaction? How do you solve this?

Answer 48

Take the equation ln[A]t = -kt + ln[A]0 plug in all the known numbers and solve algebraically remember % are decimals and the time needs to be in seconds

Question 49

For the first-order reaction, 2 N2O(g) → 2 N2(g) + O2(g), what is the concentration of N2O after 3 half-lives if mol of N2O is initially placed into a 1.00-L reaction vessel? How do you solve this?

Answer 49

Literally just divide the given moles by 2 three times This is because a half life is divided by 2