CHE 111 Final

work gained or lost by system when a gas expands form 15 L to 45 L against pressure of 1.5 atm

-4.5 kJ

use bond energies to estimate Hreaction: PCl3 +Cl -> PCl

-419 kJ

smallest mass

4.0 x 10-2 Mg

how many liters of soft drink are in 5.25 qt

4.95 L

specific heat capacity of solid copper metal is 0.385. how many joules of heat are needed to raise the temp of a 1.55 kg black of copper from 33 to 88 degrees C

3.28 x 10^4 J

what pressure will 114 g CO exert in a 3.5 L container at 75 C

4.1 atm

0.00000043 expressed correctly in scientific notation

4.3 x 10^-6

theoretical yield of HCl if 60 g of BCl3 and 37.5 g of H2O are reacted according to the equation BCl3 +3H2O -> H3BO3 +HCl

56.0 g HCl

to what temp must a balloon, at 25 C and 2 L, be heated in order to heave a volume of 6 L

894 K

solutions of NaCl and AgNO3 are mixed

AgCl precipitate forms

molecular orbital diagram most paramagnetic: B2, C2, N2

B2

change internal energy for a system that is giving off 45 kJ of heat and performing 855 J of work on surroundings

-45.9 kJ

number of sigma bonds and pi bonds in a triple bond

1 sigma, 2 pi

How many sig figs in the problem: (154.7-132) x 3.07 / 0.700

2

neutralization reaction btw Al(OH)3 and HNO3 produces salt with formula

Al(NO3)3

increasing electronegativity

Ba<Li<S

standard reaction enthalpies given below to determine Hreaction: 2NO2 +O2 -> 2NO2

-117 kJ

concentration of a solution prepared by diluting 25 mL of a stock of 0.188 M Ca(NO3)2 solution to 150 mL

0.0313 M

2.75 L container filled with CO2 gas at 25 C and 225 kPa pressure springs a leak. container resealed, pressure is 185 kPa and temp is 10 C. how many moles of gas were lost?

0.0335 mol

acid base neutralization reaction 38.74 mL of .500 M potassium hydroxide reacts with 50 mL of sulfuric acid solution. whats the concentration of H2SO4 solution?

0.194 M

2.00 moles of oxalic acid, H2C2O4 reacts with how many moles of permanganate, MnO4-

0.800 moles

mixture of 10 g of Ne and 10 g of Ar have pressure of 1.6 atm, what is partial pressure of Ne

1.1 atm

cm in 57.0 in

145 cm

what volume will a sample of gas expand if H is heated from 50 C and 2.33 L to 500 C

5.58 L

balanced equation for reaction: K3PO4 + Ca(NO3)2 -> Ca3(PO4)2 + KNO3

2K3PO4 + 3Ca(NO3)2 -> Ca3(PO4)2 + 6KNO3

complete ionic equation for reaction btw aqueous solutions of lithium sulfide and copper (II) nitrate

2Li+ + S2- + 2NO3- -> CuS(s) + 2Li+ + 2NO3-

balance equation: B2H6 + 3O2 -> B2O3 + 3H2O what is stoichiometric coefficient for oxygen

3

number of electron groups around a molecule with sp2 hybridization

3

what is the volume of 30 g of argon gas at 157 C and 2.5 kPa pressure

1070 L

convert 1.50 atm to torr

1140 torr

substance contains a nonpolar covalent bond

N2

spectator ions: NaBr + AgNO3

Na+(aq) + NO3-(aq)

compound NO2 is named

Nitrogen dioxide

element can expand valence shell to accommodate more than 8 electrons

P

wave encounters an obstacle or slit, it bends around it

diffraction

valence electrons are electrons located

in the outermost energy level of an atom

electronegativity difference btw elements X and Y is 2.1, bond is

ionic

ammonium hydroxide is a weak base because

it dissociates into ions only partially in water

meter is a measure of

length

which number contains the correct number of sig figs

156,000-- 3 sig figs

molar mass of copper (II) sulfate, CuSO4

159.6 g

tank contains mixture of helium, neon and argon partial pressure of neon

173 mmHg

double covalent bond contains

2 pairs of electrons

elements in group 2A (2) of the periodic table form ions with a charge of

2+

grams of NaCl required to make 300.0 mL of 2.500 M solution

43.83 g

wavelength of the blue light emitted by a mercury lamp with freq of 6.88 x 10^14 Hz

436 nm

mass of 2 L of an intravenous glucose solution with a density of 1.15 g/mL

2.30 kg

how many molecules of water are present in 75 g of H2O

2.51 x 10^24 molecules

how many liters of a .0550 M LiCl solution contain 0.163 moles of LiCl

2.96 L

use molecular orbital diagram to determine most stable B2C2N2

C2^2-

formula for tetraiodide

CI4

sig figs are important because they indicate

precision of a measurement

example of kinetic energy

running water

characteristic of a base

slippery, soapy feel

solution prepared by dissolving 2 g of KCl in 100 g of H2O. in this solution, H2O is the

solvent

hybridization of the C in HCN

sp

hybridization for the O in H3O+

sp3

hybridization of Br in BrCl3

sp3d

hybridization for the S in SF6

sp3d2

in which do particles move most rapidly

steam at 110 degrees C

in water, a substance that ionizes completely in solution is called a

strong electrolyte

true if Esys = -120 J

system is losing 120 J, while the surroundings are gaining 120 J

eg, mg, hybridization of NH3

tetrahedral, trigonal pyramidal, sp3

carbon tetrachloride molecule, CCl4, has shape of

tetrahedron

S + O2 -> SO2 H= -70.8 kcal which is true

70.8 kcal are produced when 32.1 g of S reacts

molar mass of potassium chloride, KCl

74.6 g

sample of 0.29 moles of Ar occupies 3.8 L under certain conditions what volume will .60 moles occupy under the same conditions

8.6 L

carbonic acid can form water and carbon dioxide upon heating. how much carbon dioxide is formed from 12.4 g of carbonic acid

8.80 g

potato contains 20 g of carbohydrate. caloric value = 4 kcal/g, how many kcal are obtained from carbohydrate in potato

80 kcal

mass of NO2 contained in 13 L tank at 4.58 atm and 385 K

87.6 g

lewis structure of BF3

F-B-F | F

oxidation states in reaction: Ca(s) + 2HI(aq) -> CaI2(aq) + H2(g)

H- reduced Ca- oxidized

correct formula for sulfuric acid is

H2SO4

identify polyprotic acid

H2SO4

neutralization reaction

HNO3 + KOH -> H2O + KNO3

symbol for the ion with 19 protons and 18 electrons

K+

mixing of which pair of reactants will result in a precipitation reaction

K2SO4(aq) + Ba(NO3)2(aq)

increasing atomic radius

Li<P<Ba

in a molecule with covalent bonding,

atoms are held together by sharing electrons

best Lewis structure for SF4

S with single pair and four single bonds to F (each with 3 lone pairs)

octet rule indicates

atoms lose, gain or share valence electrons to have 8 valence electrons

what substance is oxidized Zn + 2HCl -> ZnCl2 + H2

Zn

ground state electron config for Se

[Ar]4s2 3d10 4p4

scientific law

a brief statement that summarizes past observations and makes predictions

which polyatomic ion has a positive charge

ammonium

arrhenius concept if HNO3 were dissolved in water. it would act as

an acid

example of intensive properties

boiling points

chemical change

burning sugar

which element does not exist as a diatomic molecule

carbon

primary substances of which all other things are composed

elements

reaction that releases energy as it occurs is classified as

exothermic

how many sig figs in the answer: (8.881 x 2.100) + 0.590

four

physical property

mercury is a slivery liquid at room temp

semiconductors are

metalliods

in ionic compounds, ______ lose their valence electrons to form positively charge ________

metals, cations

give eg, mg, hybridization of XeF4

octahedral, square planar, sp3d2

according to avogardo's law

the volume of a gas is directly related to the number of moles at constant temp and pressure

shortest covalent bond

triple covalent bond

amount of space occupied by a substance is its

volume

raising temp of 10 g of water form 10 to 20 C requires 100 cal of energy while raising temp of aluminum from 10 to 20 C requires 22 cal. more calories are require to heat water cause

water has a larger specific heat than aluminum