(a)
Interpretation:
Whether the given statement is true or false needs to be determined.
In the phase diagram for a pure substance, triple point is temperature and pressure value at which the substance can boil, freeze and sublime simultaneously
Concept introduction:
Triple point is that point on the phase diagram at which all the three phases, liquid, solid and vapor, are in equilibrium with each other.
(b)
Interpretation:
Whether the given statement is true or false needs to be determined.
The boiling point of CHF3 is more than CHCl3 due to hydrogen bonding in CHCl3.
Concept introduction:
Hydrogen bond is a strong type of dipole force which act between hydrogen atoms bonded to comparatively highly electronegative atoms specially fluorine, oxygen or nitrogen atom in a molecule and an unshared pair on such atoms of the neighboring molecule. There are two types of hydrogen bonding; intermolecular and intramolecular hydrogen bonding.
(c)
Interpretation:
Whether the given statement is true or false needs to be determined.
The melting and boiling point of a compound is independent of the strength of covalent bonds in it.
Concept introduction:
Covalent bonds are intermolecular bonds which are formed by sharing of electrons between two or more atoms. These can be formed by sharing of electron/s between same or different type of atoms.
(d)
Interpretation:
Whether the given statement is true or false needs to be determined.
The pressure deceases due to decreases in the amount of a condensable gas is reduced in a tank.
Concept introduction:
Here,
P- Pressure
V-Volume
T- Temperature
n- Number of moles
R- Universal gas constant
(e)
Interpretation:
Whether the given statement is true or false needs to be determined.
The temperature above which there is only gas phase is known as the critical temperature.
Concept introduction:
The critical temperature is the temperature below which any phase of a substance can be present but above it, there is no solid and liquid phase exist. Thus, only vapor phase of the substance is present at that point.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
Chemistry: Principles and Reactions
- Use molecular structures and noncovalent interactions to explain why dimethyl ether, (CH3)2O, is completely miscible in water, but dimethylsulfide, (CH3)2S, is only slightly water soluble.arrow_forwardConsider two identical four-atom solids, one having 4 quanta of energy and the other having 10.(a) What observable property differs between these two solids?(b) Allow 3 quanta of energy to be transferred from the solid with 10 quanta to the solid with 4 quanta of energy. Determine whether this energy transfer is likely, explaining your reasoning.arrow_forwardGiven the information below, calculate the lattice enthalpy for MX(s), where M is a group 1 metal, and X is a group 17 element (standard state: X2(g)). ΔfH°(MX) = -462 kJ mol−1 ΔsubH°(M) = 127 kJ mol−1 D(X2) = 442 kJ mol−1 IE1(M) = 480 kJ mol−1 Eeg1(X) = -142 kJ mol−1 Express your answer to four significant figures. ΔlattH°(MX) = Answer kJ mol−1arrow_forward
- (a) Identify the major phases (ice, water, vapor) on the unary phase diagram of H2O below.arrow_forwardThe normal boiling point of a liquid is (a) the temperature at which the vapor pressure equals 1 atm. (b) the temperature at which the gas molecules have more kinetic energy than the molecules in the liquid. (c) the only temperature at which there can be equilibrium between liquid and gas. (d) the temperature at which the liquid will usually boil.arrow_forward6. Ethanoic acid (CH3COOH) has a much lower vapor pressure than ethanol (CH3CH2OH). What is the most reasonable explanation? (A) The polarizability of two oxygen atoms increases the London forces of attraction in ethanoic acid compared with ethanol. (B) Hydrogen bonding in ethanoic acid is the strongest attractive force and is mainly responsible for the observed data. (C) Both ethanol and ethanoic acid have an – OH, so the difference is the dipole of the second oxygen that increases the attractive forces. (D) Ethanol has an - OH group and can hydrogen bond; therefore, the London forces must cause the effect.arrow_forward
- (1) The boiling temperature of water is 100 °C at 1 atm. Its evaporation enthalpy AH is 44 kJ/mol. Use Clausius-Clapeyron equation to calculate its boiling temperature at 0.8 atm.arrow_forwardCoulombs Law describes the interaction between two charges and varies by the magnitude of these charges and inversely with the distance between them. For atoms, we'll label the charges as the nuclear charge and electron charge. 9192 9nuclelec As you go up in atomic number (Z), the number of protons in the nucleus increases, making the charge on the nucleus increase, so that in general. qnuc = Z ·(+1) However if we think only of the electrons in the outermost shells (valence electrons), they do not see the full strength of the nuclear charge because it is partially shielded (or canceled out if you prefer) by the core electrons. So we define something called effective charge. Shielding Experiences net charge of about 1+ Nucleus Effective Charge = # of protons Zeff = Z – core # of core electrons In general, Zeff increases as you go across in the periodic table. 1. Fill out the following table to verify that effective charge increases as you go across a row. Element Na Mg Al Si P S CI Ar…arrow_forward(a) Consider a substance where the intermolecular forces hold the molecules in fixed rigid positions. What is the process called when enough heat has been added to the substance so that the molecules begin to flow? (b) Consider a substance where the intermolecular forces hold the molecules in close contact with each other, but the molecules can flow. What is the process called when enough heat has been added to the substance so that the molecules escape each other? (c) Consider a substance where the intermolecular forces hold the molecules in fixed rigid positions. What is the process called when enough heat has been added to the substance so that the molecules can escape each other?arrow_forward
- (a) Place the following substances in order of increasingvolatility: CH4, CBr4, CH2Cl2, CH3Cl, CHBr3, and CH2Br2.(b) How do the boiling points vary through this series?(c) Explain your answer to part (b) in terms of intermolecularforces.arrow_forwardExplain (i) The basis of similarities and differences between metallic and ionic crystals.arrow_forwardThe AHvap of xenon is 12.57 kJ · mol¬' and its ASvan is 76.15 J · mol¬1 . K-l. What it the boiling point of xenon? Th = °Carrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning