Learn more about our help with Assignments: Chemistry
Search & Filtering
Which of the following is not true?
Hydrogen bonding helps explain why solid water floats on liquid water.
Hydrogen bonding is responsible for the relatively low boiling point of water.
Water molecules are farther apart in solid water than they are in liquid water.
Hydrogen bonding is responsible for the relatively high boiling point of water.
Hydrogen bonding helps explain why solid water floats on liquid water.
Hydrogen bonding is responsible for the relatively low boiling point of water.
Water molecules are farther apart in solid water than they are in liquid water.
Hydrogen bonding is responsible for the relatively high boiling point of water.
Which of the following is not true?
Deoxyribonucleic acid is stabilized by hydrogen bonds and London dispersion forces.
van der Waals forces can exist between two different parts of the same large molecule.
The level of protein structure that is stabilized by London dispersion forces is called the secondary structure.
The level of protein structure that is stabilized by London dispersion forces is called the tertiary structure
Deoxyribonucleic acid is stabilized by hydrogen bonds and London dispersion forces.
van der Waals forces can exist between two different parts of the same large molecule.
The level of protein structure that is stabilized by London dispersion forces is called the secondary structure.
The level of protein structure that is stabilized by London dispersion forces is called the tertiary structure
Which of the following is true?
Hydrogen bonds are stronger than covalent bonds.
A hydrogen bond is an electrostatic attraction between the nucleus of a hydrogen atom, bonded to fluorine, oxygen, or nitrogen, and the positive end of a nearby dipole.
In liquid water, each water molecule is hydrogen bonded to two other water molecules.
Hydrogen bonding is one type of dipole-dipole interaction
Hydrogen bonds are stronger than covalent bonds.
A hydrogen bond is an electrostatic attraction between the nucleus of a hydrogen atom, bonded to fluorine, oxygen, or nitrogen, and the positive end of a nearby dipole.
In liquid water, each water molecule is hydrogen bonded to two other water molecules.
Hydrogen bonding is one type of dipole-dipole interaction
Methanol, ethanol, ammonia, and methylamine are soluble in water because
they can form ion-induced dipoles
they can form hydrogen bonds
there are dipole-dipole forces
there are dispersion forces
they can form ion-induced dipoles
they can form hydrogen bonds
there are dipole-dipole forces
there are dispersion forces
A 0.582-mil sample of an ideal gas is at 15degrees Celsius and 81.8kPa. Calculate the volume for the ideal gas as described by the ideal gas law
The nature of the reactants is a factor affect rate because: check all that applies
a) some molecules are not symmetrical
b)some molecules have higher energy bonds
c)dissolved ions tend to have a faster rate of reaction
d)dissolved ions tend to attract each other
a) some molecules are not symmetrical
b)some molecules have higher energy bonds
c)dissolved ions tend to have a faster rate of reaction
d)dissolved ions tend to attract each other
A reaction is found to be second order with respect to reactant A. What would be the effect on the rate if the concentration of A were doubled?
A. The rate would be double
B. The rate would quadruple
C. The rate would decrease by half
D. The rate would increase in an unpredictable way
E. The concentration of A has no effect on the rate
A. The rate would be double
B. The rate would quadruple
C. The rate would decrease by half
D. The rate would increase in an unpredictable way
E. The concentration of A has no effect on the rate
If the rate law for a hypothetical reaction is r = k[A]^2[B]^1, what is the order of reaction with respect to A?
A sample weighing 4.52g containing KHP (MM=204.2 g/mol) required 28 ml of 0.15M NaOH solution for neutralization, calculate the mass percent of KHP in this sample
4. Solubility products for a series of iodides are:
AgI Ksp = 8.3 x 10-17
PbI2 Ksp = 7.1 x 10-9
BiI3 Ksp = 8.1 x 10-19
List these three compounds in order of decreasing (from highest to lowest) molar solubility in:
a. Water
b. 0.10 M NaI
AgI Ksp = 8.3 x 10-17
PbI2 Ksp = 7.1 x 10-9
BiI3 Ksp = 8.1 x 10-19
List these three compounds in order of decreasing (from highest to lowest) molar solubility in:
a. Water
b. 0.10 M NaI
