WorksheetsChap 5 - 9 Review Paper 1 Q's
Total questions: 40
Worksheet time: 2hrs 44mins
What is the volume of steam produced when 1.00 g of ice is heated to 323 degrees Celsius at a pressure of 101 kPa
0.27 dm3
1.3 dm3
2.7 dm3
48 dm3
Solid carbon dioxide, CO2, is similar to solid iodine, I2, in its structure and properties. Carbon is in Group 14. Silica, SiO2 is a group 14 compound. Which statement about solid CO2 and solid SiO2 is correct?
Both solids exist in a lattice structure.
Both solids have a simple molecular structure.
Both solids have atoms joined by single covalent bonds.
Both solids change spontaneously to gas at s.t.p.
An article in a science magazine contains the following statement. 'It is lighter than a feather, stronger than steel, yet incredibly flexible and more conductive than copper'. Which form of carbon is being described?
Buckminsterfullerine
Diamond
Graphene
Graphite
Which equation has an enthalpy change of reaction which corresponds to the enthalpy change of atomization of Chlorine?
1/2 Cl2(g) --> Cl(g)
1/2 Cl2(l) --> Cl(g)
Cl2(g) --> 2 Cl(g)
Cl2(l) --> 2 Cl(g)
In an experiment, 2.00 mol of hydrogen and 3.00 mol of iodine were heated together in a sealed container and allowed to reach equilibrium at a fixed temperature. The container had a fixed volume of 1.00 dm3. At equilibrium there were 2.40 moles of iodine present in the mixture.
Equation : H2(g) + I2(g) <--> 2 HI(g)
What is the value of the equilibrium constant, Kc ?
0.107
0.357
0.429
2.33
Which statement(s) about reversible reactions are correct?
1 An increase in concentration of a reactant always increases the concentration of the product
2 An increase in temperature always increases the rate at which equilibrium is established
3 An increase in temperature always increases the amount of the product at equilbrium
1, 2 and 3 are correct
1 and 2 are correct
2 and 3 are correct
only 1 is correct
A chemist puts a sample of dilute aqueous hydrochloric acid into beaker 1. She adds a sample of zinc and measures the rate of production of hydrogen gas.
She then puts a different sample of dilute aqueous hydrochloric acid into beaker 2. She adds a different sample of zinc and measures the rate of production of hydrogen gas.
The rate of reaction in beaker 2 is greater than that in beaker 1.
Which factors could help explain this observation?
The reaction in beaker 1 has a higher activation energy than the reaction in beaker 2.
The zinc in beaker 1 is in larger pieces than the zinc in beaker 2.
The acid in beaker 1 is at a lower concentration than the acid in beaker 2.
Solid sulfur consists of molecules made up of eight atoms covalently bonded together. The bonding in sulfur dioxide is O=S=O.
Enthalpy change of combustion of S8 = -2376 kJ/mol
Energy required to break 1 mole S8(s) into gaseous atoms = 2232 kJ/mol
O=O bond enthalpy = 496 kJ/mol
Using this data , what is the value of the S=O bond enthalpy?
239 kJ/mol
257 kJ/mol
319 kJ/mol
536 kJ/mol
In an experiment, the burning of 1.45 g (0.025 mol) of propane was used to heat 100 g of water. The initial temperature of the water was 20.0 degrees Celsius and the final temperature of the water was 78.0 degrees Celsius. Which experimental value for the enthalpy change of combustion for propanone can be calculated from these results?
-1304 kJ/mol
-970 kJ/mol
-352 kJ/mol
-24.2 kJ/mol
A mixture of nitrogen and hydrogen gases, at a temperature of 500 K, was put into an evacuated vessel of volume 6 dm3. The vessel was then sealed.
Equation N2(g) + 3 H2(g) <--> 2 NH3(g)
The mixture was allowed to reach equilibrium. It was found that 7.2 mol of N2 and 12.0 mol of H2 were present in the equilibrium mixture. The value of the equilibrium constant, Kc , for this equilibrium is .06 at 500 K.
What is the concentration of ammonia present in the equilibrium mixture at 500 K?
0.58 mol / dm3
0.76 mol / dm3
3.5 mol / dm3
27 mol / dm3
Ammonia is made by the Haber process. The reactants are nitrogen and hydrogen.
N2(g) + 3 H2(g) <--> 2 NH3(g) (Exothermic Reaction)
What will increase the rate of the forward reaction?
Adding argon to the mixture but keeping the total volume constant.
Decreasing the temperature.
Increasing the total pressure by reducing the total volume at constant temperature.
Removing ammonia as it is made but keeping the total volume of the mixture the same.
A sample of iodine vapour of mass 6.35 g has a volume of 1.247 dm3 when maintained at constant temperature and a pressure of 1.00 x 105Pa.
If iodine vapour acts as an ideal gas, what is the temperature of the iodine vapour?
300 K
600 K
300 000 K
600 000 K
A student mixed 25.0 cm3 of 0.350 mol dm-3 sodium hydroxide solution with 25.0 cm3 of 0.350 mol dm-3 hydrochloric acid . The temperature rose by 2.50 degrees Celsius. Assume that no heat was lost to the surroundings. The final mixture had a specific heat of 4.2 J cm-3 K-1.
What is the molar enthalpy change for the reaction?
-150 kJ/mol
-60 kJ/mol
-30 kJ/mol
-0.150 kJ/mol
(Hint: You will need to make a chemical equation to solve)
The enthalpy change of formation of carbon dioxide is -394 kJ/mol
The enthalpy change of formation of water is -286 kJ/mol
The enthalpy change of formation of methane is -74 kJ/mol
What is the enthalpy change of combustion of methane?
-892 kJ/mol
-606 kJ/mol
+606 kJ/mol
+892 kJ/mol
Hydrogen and carbon dioxide gases are mixed in equal molar amounts at 800 K. A reversible reaction takes place.
H2(g) + CO2(g) <--> H2O(g) + CO(g)
At equilibrium the partial pressures of H2 and CO2 are both 10.0 kPa. Kp is 0.288 at 800 K. What is the partial pressure of CO in the equilibrium mixture?
5.37 kPa
18.6 kPa
28.8 kPa
347 kPa
In which reaction is the species in italics acting as an oxidizing agent?
2 Ca + O2 --> 2 CaO
Cr2O72- + 8 H+ + 3 SO32- --> 2 Cr3+ + 4 H2O + 3 SO42-
Mg + Fe2+ --> Mg2+ + Fe
SO2 + 2 H2O + 2 Cu2+ + 2 Cl- --> H2SO4 + 2 H+ + 2 CuCl
The formation of hydrogen and ethyne, C2H2, from methane reaches dynamic equilibrium.
2 CH4(g) <--> 2 H2(g) + C2H2(g)
What are the units of Kc?
mol dm-3
mol2dm-6
mol3dm-9
mol4dm-12
Which equation represents the standard enthalpy change of formation of ethanol, C2H5OH?
2C(g) + 3H2(g) + 1/2 O2(g) --> C2H5OH(l)
2C(s) + 3H2(g) + 1/2 O2(g) --> C2H5OH(l)
2C(s) + 3H2(g) + 1/2 O2(g) --> C2H5OH(g)
2C(g) + 6H(g) + O(g) --> C2H5OH(g)
Sulfuric acid is a Bronsted-Lowry Acid. In which reactions is sulfuric acid behaving as an acid?
H2SO4 + HNO3 --> H2NO3+ + HSO4-
H2SO4 + CO32- --> CO2 + H2O + SO42-
H2SO4 + MgO --> MgSO4 + H2O
In which reaction does hydrogen behave as an oxidizing agent?
H2 + Cl2 --> 2 HCl
C2H4 + H2 --> C2H6
N2 + 3 H2 --> 2 NH3
2 Na + H2 --> 2 NaH
For which equation is the enthalpy change correctly described as an enthalpy change of formation?
C(g) + O2(g) --> CO2(g)
C(s) + 1/2 O2(g) --> CO(g)
2N(g) + 4O(g) --> N2O4(g)
2 NO(g) + O2(g) --> 2 NO2(g)
In an experiment to calculate the enthalpy change of combustion of a fuel, 1.5 g (0.0326 mol) of the fuel was used to heat 200 g of water. The temperature of the water rose from 25 to 55 degrees Celsius. The specific heat capacity of water is 4.18 J / g*K. There is significant heat loss in this experiment. Therefore, the experimental value for the enthalpy change of combustion of the fuel will be different from the theoretical value.
Using the information above, what is the experimental value for the enthalpy change of combustion (in kj mol- of the fuel).
-1410
-769
-30.7
-16.7
A reversible reaction is catalyzed.
Which statements about the effects of the catalyst on this system are correct?
The catalyst alters the mechanism of the reaction
The catalyst reduces the activation energy for both the forward and the backward reaction
The catalyst alters the composition of the equilibrium mixture
A student borrowed a friend's chemistry notes and copied the notes in the box below. Which statements are correct?
A gas behaves less like an ideal gas when?
it is at low pressure
it is at low temperature
it can be easily liquefied
Hydrogen Sulfide is released from volcanoes. It reacts with oxygen in the air to form sulfur dioxide.
2 H2S(g) + 3 O2(g) --> 2 H2O(l) + 2 SO2(g)
Enthalpy of Formation H2S = - 21 kJ/mol
Enthalpy of formation H2O = - 286 kJ/mol
Enthalpy of Formation SO2 = -297 kJ/mol
What is the standard enthalpy change of reaction in kJ/mol
-1208
-1124
-562
-541
When 0.47 g of a hydrocarbon was completely burnt in air, the energy released 200 g of water from 23.7 to 41.0 degrees Celsius.
What was the amount of energy absorbed by the water?
0.47 x 4.18 x 17.3 J
0.47 x 4.18 x (273 + 17.3) J
200 x 4.18 x 17.3 J
200 x 4.18 x (273 +17.3) J
Copper and iodine are both shiny crystalline solids. Which forces exist between particles in solid copper and between neighboring iodine molecules in solid iodine?
Copper: ionic bonds Iodine: covalent bonds
Copper: ionic bonds Iodine: van Der waals
Copper: metallic bonds Iodine: covalent bonds
Copper: metallic bonds Iodine: van Der wall's forces
In a solution that contains both Br2 and Cl2 , a process takes place that produces BrO3- ions. The process is represented by the following equations.
equation 1: Br2 + H2O --> HBr + HBrO
equation 2: 3 HBrO + Cl2 --> 2 Cl- + BrO3- + Br2 + 3 H+
Chlorine is reduced in equation 2
Bromine is oxidized in both equation 1 and equation 2
Bromine is reduced in both equation 1 and equation 2
Which names can be applied to the enthalpy change of the reaction shown below?
H2(g) + 1/2 O2(g) --> 2 H2O(l)
enthalpy change of formation
enthalpy change of combustion
enthalpy change of hydration
In oxygen difluroide, OF2, fluorine has an oxidation number of -1. OF2 will react with sulfur dioxide according to the following equation: OF2 + SO2 --> SO3 + F2
What is oxidized and what is reduced in this equation?
Oxidized: Fluorine and oxygen in OF2 Reduced: Sulfur
Oxidized: Fluorine and Sulfur Reduced: Oxygen in OF2
Oxidized: Oxygen in OF2 Reduced: Fluorine and Sulfur
Oxidized: Sulfur Reduced: Fluorine and Oxygen in OF2
The gas laws can be summarized in the ideal gas equation below.
pV=nRT
0.96 g of oxygen gas is contained in a glass vessel of .007 m3 at a temperature of 30 degrees celsius.
Assume the gas behaves as an ideal gas.
What is the pressure in the vessel?
1.1 kPa
2.1 kPa
10.8 kPa
21.6 kPa
One mole of phosphorous (V) chloride is heated to 600 K in a sealed flask of volume 1 dm3.
PCl5(g) <--> PCl3(g) +Cl2(g)
The experiment is repeated with one mole of phosphorous chloride heated to 600 K in a sealed flask of volume 2 dm3.
How will the measurements vary?
The equilibrium concentration of PCl3(g) and Cl2(g)will be higher in the second experiment
The equilibrium concentration of PCl5 will be lower in the second experiment.
The equilibrium concentrations of all three gases are the same in both experiments.
The value of the equilibrium constant is higher in the second experiment.
In which reaction is the underlined substance acting as a base?
HNO3 + H2SO4 --> H2NO3+ + HSO4-
HSiO3 + HCN --> CN- + H2O + SiO2
HNO2 + HCO3- --> H2O + CO2 + NO2-
C6H5O- + CH2ClCO2H --> C6H5OH + CH2ClCO2-
Nitrogen dioxide, NO2 , exists in equilibrium with dinitrogen tetroxide, N2O4.
2 NO2(g) <--> N2O4(g) Enthalpy of reaction = - 57 kJ/mol
Which conditions give the greatest percentage of N2O4(g) at equilibrium?
Pressure : high Temperature: high
Pressure: high Temperature: low
Pressure: low Temperature: high
Pressure: low Temperature: low
When a sample of HI is warmed to a particular temperature the equilibrium below is established.
2 HI(g) <--> H2(g) + I2(g)
At this temperature, it is found that the partial pressure of HI is 28 times the partial pressure of H2. What is the value of Kp at this temperature?
1.28 x 10-3
0.035
28
784
Which statements are correct for all exothermic reactions?
The enthalpy for the reaction is negative.
On a reaction pathway diagram the products are shown lower than the reactants.
The reaction will happen spontaneously.
Which of these reactions are redox reactions?
6 NO(g) + 4 NH3(g) --> 5 N2(g) + 6 H2O(g)
2 SO2(g) + O2(g) --> 2 SO3(g)
SO3(g) + H2O(g) --> H2SO4(g)
What is a basic assumption of the kinetic theory, as applied to an ideal gas?
Collisions between gas molecules are elastic.
Each molecule occupies a finite volume.
Gases consist of particles that experience the force of gravity.
Gas molecules attract each other with weak intermolecular forces.
In this question you should assume that all gases behave ideally. Hydrogen and iodine react reversibly in the following reaction. The system reaches equilibrium.
H2(g) + I2(g) <--> 2HI(g). Enthalpy of reaction = -9.5 kJ/mol
Which statement must be true for Kp to stay constant?
The partial pressures of all gases are equal.
The external pressure is constant.
The forward and reverse reactions have stopped.
The temperature is constant.
Two reactions are shown.
Reaction 1 N2(g) + 3 H2(g) <--> 2 NH3(g)
Reaction 2 2 O3(g) <--> 3 O2(g)
In reaction 1 a finely powdered iron catalyst is used.
In reaction 2 a vaporized tetrachloromethane catalyst in ultraviolet light is used.
Which statement about the catalysts used is correct?
Both reaction 1 and reaction 2 use a homogenous catalyst.
Both reaction 1 and reaction 2 use a heterogeneous catalyst.
Reaction 1 : heterogenous catalyst Reaction 2: homogenous catalyst
Reaction 1: homogenous catalyst Reaction 2: heterogenous catalyst
