Concept explainers
(a)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
According to phase diagram, the three phases of any substance is inter convertible in between. The solid can be converted into liquid by heating it up to its melting point and the process is known as melting or fusion.
(b)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
According to phase diagram, the three phases of any substance is interconvertible in between. The liquid can be converted into gaseous form by heating it up to its boiling point and the process is known as boiling.
(c)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
According to phase diagram, the three phases of any substance is interconvertible in between. The solid can be converted into liquid by heating it up and liquid is further into in to gaseous form by adding continues heat until it reaches to its boiling point.
(d)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
According to heating curve, heat of fusion is a heat applied to a 1.0 g of solid substance to convert it in to its liquid phase.
(e)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Heating curve describes that the amount of heat required to vaporize 1.0 g of liquid at its normal boiling point is called as Heat of vaporization.
(f)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
The heat of vaporization is the amount of heat that is required to evaporate 1.0 g of liquid to gas form at its normal boiling point.
(g)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Heat of vaporization is the amount of heat required to evaporate 1.0 g of liquid to gas at its normal boiling point. The amount of heat is required to convert 1.0 g of solid to its liquid form is called as Heat of fusion.
(h)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Melting is a process in which the solid is heated to its melting point and gets converted into liquid. Crystallization is a process in which liquid is cooled to temperature to form a solid form of it.
(i)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Exothermic process is a process during which system releases energy whereas endothermic process is a process during which system absorbs energy.
(j)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Melting is a process in which the solid is heated to its melting point and gets converted into liquid. This liquid formed from solid have the same molecules in it. For getting solid once again, liquid is required to be cooled back.
(k)
Interpretation:
To justify whether the given statement is true or false.
Concept Introduction:
Sublimation is a process in which a direct formation of gas form from solid form of substance occurs.
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Chapter 5 Solutions
Introduction to General, Organic and Biochemistry
- Define the joule in terms of SI base units.arrow_forwardIf 14.5 kJ of heat were added to 485 g of liquid water, how much would its temperature increase?arrow_forward9.46 The heat of fusion of pure silicon is 43.4 kJ/mol. How much energy would be needed to melt a 5.24-g sample of silicon at its melting point of 1693 K?arrow_forward
- Are changes in state physical or chemical changes? Explain. What type of forces must be overcome to melt or vaporize a substance (are these forces intramolecular or intermolecular)? Define the molar heat of fusion and molar heat of vaporization. Why is the molar heat of vaporization of water so much larger than its molar heat of fusion? Why does the boiling point of a liquid vary with altitude?arrow_forward5-86 Using the phase diagram of water (Figure 5-20), describe the process by which you can sublime 1 g of ice at-10°C and at 1 atm pressure to water vapor at the same temperature.arrow_forwardA representation of liquid water is shown below. Which of the three representations that follow best describes the water after it has boiled into steam?arrow_forward
- The amount of heat required to melt 2 lbs of ice is twice the amount of heat required to melt 1 lb of ice. Is this observation a macroscopic or microscopic description of chemical behavior? Explain your answer.arrow_forwardIn each of the following groups of substances, pick the one that has the given property. Justify your answer. (a) highest boiling point Ne C12₂ HI Since this compound has ---Select--- (b) highest freezing point NH3 H₂O KCI Since this compound has ---Select--- unlike the other two compounds, it has the ---Select--- unlike the other two compounds, it has the ---Select--- (c) lowest vapor pressure at 25°C C12 12 F₂ Since all the molecules are ---Select--- and this molecule is ---Select--- than the other two, it has the intermolecular forces and will have the highest boiling point. intermolecular forces and will have the highest freezing point. ---Select--- ↑ ---Select--- (d) lowest freezing point H₂Se H₂ Cse2 Since this molecule is ---Select--- and ---Select--- than the other two, it has the ---Select--- ♥ ---Select--- and will have the lowest vapor pressure. and will have the lowest freezing point.arrow_forwardAs a substance is subjected to pressure and/or temperature changes, it may undergo condensation, deposition, freezing, melting, sublimation, or vaporization. (a) Consider the phase diagram shown below and state the cha nges that take place upon going from points A to B to C to D. (b) Is the transition from C to D exothermic or endothermic?arrow_forward
- Explain why water boils at higher temperature under higher pressure (pure substance saturation temperature depends on pressure). Use knowledge of energy and energy transferring at molecular or atomic level during the phase change of a substance. You do not need to show calculations. • (a) the amount of heat absorbed as 1 kg of saturated liquid water boils at 100°C. (b) the amount of heat released as 1 kg of saturated water vapor condenses. Is a >b, a=b, or aarrow_forwardCalculate the heat released when 65.5g of water at 55.5 ° C cools to ice at 0.0 ° C. (Given that the specific heat of liquid water is 1.00 calg×°C, and heat of water solidification is 80.0 cal/g.).arrow_forward3. True or false: Because dry ice sublimes, carbon dioxide has no liquid phase. (a) True (b) Falsearrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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