AS & A Level Chemistry - 9701 Paper 1 2012 Summer Zone 3

Ammonia is manufactured by the Haber Process, in an exothermic reaction.
Assuming that the amount of catalyst remains constant, which change will not bring about an increase in the rate of the forward reaction?

In which species does the underlined atom have an incomplete outer shell?

The value of the second ionisation energy of calcium is 1150 kJ mol\(^{-1}\).
Which equation correctly represents this statement?

The equation for a reaction is shown.

$\text{H}_2(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{H}_2\text{O}(l) ; \Delta H = x \text{ kJ mol}^{−1}$

Which pair of descriptions is fully correct for this reaction?

[Table_1]

Propanone has the molecular formula $C_3H_6O$.
The enthalpy change of combustion of hydrogen is $-286\,\text{kJ}\,\text{mol}^{-1}$.
The enthalpy change of combustion of carbon is $-394\,\text{kJ}\,\text{mol}^{-1}$.
The enthalpy change of combustion of propanone is $-1786\,\text{kJ}\,\text{mol}^{-1}$.
Using this information, what is the enthalpy change of formation of propanone?

Two conversions are outlined below.
$$\text{NH}_4^+ \rightarrow \text{NH}_3$$
$$\text{C}_2\text{H}_4 \rightarrow \text{C}_2\text{H}_6$$
What similar feature do these two conversions have?

Use of the Data Booklet is relevant to this question.
The gas laws can be summarised in the ideal gas equation.

$pV = nRT$

0.56 g of ethene gas is contained in a vessel at a pressure of 102 kPa and a temperature of 30°C.
What is the volume of the vessel?

Under which set of conditions is a gas most likely to behave ideally?
[Table_1]

The diagram shows a cell for the manufacture of aluminium.

Which statement is incorrect?

The oxide of titanium, $\text{TiO}_2$, is used as a 'whitener' in toothpaste. It is obtained from the ore iron(II) titanate, $\text{FeTiO}_3$.
What is the change, if any, in the oxidation number (oxidation state) of titanium in the reaction $\text{FeTiO}_3 \rightarrow \text{TiO}_2$?

Two moles of compound P were placed in a vessel. The compound P was partly decomposed by heating. A dynamic equilibrium between chemicals P, Q and R was established.
At equilibrium, x mol of R were present and the total number of moles present was $(2 + x)$.
What is the equation for this equilibrium?

When a mineral was heated in a Bunsen flame to constant mass, a colourless gas that turned lime water milky was evolved. The remaining solid was cooled and then added to aqueous hydrochloric acid. Vigorous effervescence was seen.
What was the mineral?

Aluminium chloride catalyses certain reactions by forming carbocations with chloroalkanes as shown.
$$\text{RCl} + \text{AlCl}_3 \rightarrow \text{R}^+ + \text{AlCl}_4^-$$
Which property makes this reaction possible?

The oxides BaO, CaO, MgO and SrO all produce alkaline solutions when added to water.
Which oxide produces the saturated solution with the highest pH?

Use of the Data Booklet is relevant to this question.
The reaction between aluminium powder and anhydrous barium nitrate is used as the propellant in some fireworks. The metal oxides and nitrogen are the only products.
Which volume of nitrogen, measured under room conditions, is produced when 0.783 g of anhydrous barium nitrate reacts with an excess of aluminium?

The following two experiments are carried out with anhydrous potassium chloride and observations X and Y are made at the end of each experiment.

Concentrated sulfuric acid is added to the potassium chloride and the fumes produced are bubbled into aqueous potassium iodide solution - observation X.

The potassium chloride is dissolved in aqueous ammonia and this is then added to aqueous silver nitrate - observation Y.

What are the observations X and Y?

[Table_1]

In the treatment of domestic water supplies, chlorine is added to the water to form $\text{HClO}$.
$\text{Cl}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightarrow \text{H}^+(\text{aq}) + \text{Cl}^-(\text{aq}) + \text{HClO}(\text{aq})$
The $\text{HClO}$ reacts further to give $\text{ClO}^-$ ions.
$\text{HClO}(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightarrow \text{H}_3\text{O}^+(\text{aq}) + \text{ClO}^-(\text{aq})$
Both $\text{HClO}$ and $\text{ClO}^-$ kill bacteria by oxidation.
What is the overall change in oxidation number of chlorine when forming the $\text{ClO}^-$ ion from the aqueous chlorine?

What trend is observed on descending Group VII?

Fumaric acid can be converted into oxaloacetic acid by a two-step process involving the intermediate $Q$.

$$\text{HO}_2\text{CCH=CHCO}_2\text{H} \xrightarrow{\text{step 1}} Q \xrightarrow{\text{step 2}} \text{HO}_2\text{CCOCH}_2\text{CO}_2\text{H}$$

Each of these steps can be achieved in the laboratory by a single reagent.
What could be the intermediate $Q$ and the reagent for step 2?

Carbon monoxide, CO, nitrogen monoxide, NO, and sulfur dioxide, SO\textsubscript{2}, may all be present in the exhaust fumes from a car engine.
Which reaction concerning these compounds occurs in the atmosphere?

An organic compound $J$ reacts with sodium to produce an organic ion with a charge of $-3$. $J$ reacts with NaOH(aq) to produce an organic ion with a charge of $-1$.
What could be the structural formula of $J$?

Compound C is used in textile and leather processing.
Which starting material(s), on gentle heating with a few drops of concentrated sulfuric acid, generates compound C?

How many isomeric esters have the molecular formula $C_4H_8O_2$?

A sample of ethyl propanoate is hydrolysed by heating under reflux with aqueous sodium hydroxide. The two organic products of the hydrolysis are separated, purified and weighed. Out of the total mass of products obtained, what is the percentage by mass of each product?

Which of these compounds can be oxidised by acidified dichromate(VI) solution and also gives a positive response to Tollens’ reagent?
CH₃COCH₂CH₂OH \: W
CH₃COCH₂CHO \: X
CH₃CH(OH)CH₂CH₃ \: Y
CH₃CH₂CH₂CHO \: Z

Which compound, on reaction with hydrogen cyanide, produces a compound with a chiral centre?

The depletion of the ozone layer in the upper atmosphere reduces the Earth's natural protection from harmful ultraviolet radiation.
Which compound would cause the most depletion of the ozone layer?

The presence of halogen in an organic compound may be detected by warming the organic compound with aqueous silver nitrate.
Which compound would produce a precipitate quickest?

A reaction pathway diagram is shown.

Which reaction does not have such a profile?

Which statement does not correctly describe the polymer PVC?

Nitrogen and phosphorus are both in Group V of the Periodic Table. Phosphorus forms a chloride with the formula $\text{PCl}_5$.
Why is it not possible for nitrogen to form $\text{NCl}_5$?
1. Nitrogen’s outer shell can only contain eight electrons.
2. Nitrogen cannot have oxidation state $+5$.
3. Nitrogen is almost inert.

Use of the Data Booklet is relevant to this question.
In which pairs do both species have the same number of unpaired p electrons?

The gas laws can be summarised in the ideal gas equation.

$pV = nRT$

where each symbol has its usual meaning.
Which statements are correct?
1. One mole of an ideal gas occupies the same volume under the same conditions of temperature and pressure.
2. The density of an ideal gas at constant pressure is inversely proportional to the temperature, $T$.
3. The volume of a given mass of an ideal gas is doubled if its temperature is raised from 25°C to 50°C at constant pressure.

Which statements are correct for all three halogens, chlorine, bromine and iodine?
1. They all form hydrides that are strong acids in aqueous solution.
2. They all react with aqueous sodium hydroxide to form oxo-anions.
3. They all require one more electron to fill the $p$ orbitals of their outer shells.

In the manufacture of sulfuric acid the reaction $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$ usually takes place at 400 °C and 1 atm pressure. In one industrial plant, it is decided to change the pressure to 20 atm.
What will be the consequences of this change?
1. increased running costs
2. an increased percentage of sulfur trioxide in the equilibrium mixture
3. the rate of the backward reaction increases

Ammonia and chlorine react in the gas phase.

$$8NH_3 + 3Cl_2 \rightarrow N_2 + 6NH_4Cl$$

Which statements are correct?
1. Ammonia behaves as a reducing agent.
2. Ammonia behaves as a base.
3. The oxidation number of the hydrogen changes.

A number of alcohols with the formula $C_4H_{10}O$ are separately oxidised. Using 70 g of the alcohols, a 62% yield of organic product is achieved. What mass of product could be obtained?

What is always involved in a carbon-carbon $\pi$ bond?

How can a good yield of ethylamine be made using bromoethane as starting material?

Which reagents will react with cis-hex-3-enal?
cis-hex-3-enal
1. sodium
2. sodium borohydride
3. Fehling's reagent