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Q3-SUMMATIVE TEST IN GEN. CHEMISTRY 2
Quiz by Hazel Castro
Tag the questions with any skills you have. Your dashboard will track each student's mastery of each skill.
The principal source of difference in the normal boiling points of ICI (97Â oC; mol. mass 162 amu) and Br2 (59 oC; mol. mass 160 amu) is:
Of the following substances, only _______has London-dispersion forces as the only intermolecular force.
Of the following diatomic molecules, which has the highest boiling point?
Which statements about viscosity is true?
(i) Viscosity increases as temperature decreases.
(ii) Viscosity increases as molecular weight increases.
(iii) Viscosity increases as intermolecular force increase.
Which of the following diatomic molecules has the highest heat of vaporization?
In general, the vapor pressure of a substance increases as _________ increases.
Which group of substances is arranged in order from the highest to the lowest melting point?
When the electron cloud of a molecule is easily distorted, the molecule has a high ________________.
When liquid bromine is cooled to form a solid, which of the following types of solid would it form?
The stronger the intermolecular forces in a substance...
Where is the point on the phase diagram where the substance exists as solid, liquid, and gas?
On a phase diagram, the temperature and pressure at which the phase boundary between the liquid and gas ceases to exist. What is it called?
What is the phase of the substance that goes beyond the critical point?
During these phase changes, which did NOT release energy?
Which of the following is an example of sublimation?
Which of the following cannot be obtained using a phase diagram?
Which of the following is TRUE about the phase diagram of Carbon dioxide?
A pure solid substance is heated as indicated in the diagram below. What line segment represents the solid state?
What phase change occurs at line segment BC?
At what line segment is the substance vaporizing?
What is the freezing point of an aqueous 1.00 m NaCl solution? Kf = 1.86 °C/m
Which of the following aqueous solutions will have the lowest freezing point?
How is boiling point elevation presented in an equation?
How are vapor pressure and boiling point elevation related?
Given the following solutions, 3 m C6H12O6, 2 m NaCl, 0.5 m Mg(OH)2 m, what is the correct arrangement in terms of increasing boiling point?
Which of the following observations reflects colligative properties?
I. A 0.5 m NaOH solution freezes at a lower temperature than pure water.
II. Pure water freezes at a higher temperature than pure methanol.
Which of the following is an example of exothermic reaction?
What work is done on the system, if it releases 50 J of heat and there is an increase of 25 J internal energy?
What type of reaction is photosynthesis, and what is the value of ∆H?
What is the net internal energy of a system if it absorbs 30 kJ of heat and does 10 kJ of work?
Which of the following statements best describes the rate of a chemical reaction?
What do you call the minimum amount of energy required for a chemical reaction to occur?
Raw carrots are cut into thin slices for cooking.
Consider the following equation. Mg + 2HCl → MgCl2 + H2. If 120 cm3 of hydrogen is formed in 60 s, what is its rate of reaction?
∆H for the reaction IF5 (g) --> IF3 (g) + F2 (g) is ________ kJ, given the data below.
IF (g) + F2 (g) --> IF3 (g) ∆H = - 390 kJ
IF (g) + 2 F2 (g)--> IF5 (g) ∆H = - 745 kJ
The value of ∆H° for the reaction below is -72 kJ. How many kJ of heat are released when 1.0 mol of HBr is formed in this reaction?
H2 (g) + Br2 (g) --> 2HBr (g)
What is the molality of phosphoric acid, H3PO4, in a solution of 14.5 g of H3PO4 in 125 g of water?
Which of the following describes what happens when you hold an ice cube in your hand?
Which of the following is NOT true about Hess’s law?
Which of the following statement is TRUE once a hot flat iron is unplugged and starts to cool?