How to Join PN Cadet: A Complete Step-by-Step Guide
If you’re looking to join PN Cadet, it’s essential to understand both the requirements and the opportunities this prestigious program offers. The Pakistan Navy provides an excellent pathway for young individuals to serve their country while gaining top-tier education and training. To join PN Cadet, candidates must meet certain eligibility criteria, including age, educational qualifications, and physical standards.
Once selected, you’ll undergo rigorous training that prepares you for a rewarding career in the Navy. The program not only offers a chance to serve but also provides valuable leadership experience, technical skills, and opportunities for advancement within the armed forces. If you’re committed, disciplined, and passionate about contributing to national security, joining PN Cadet could be the perfect career choice.
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Q. According to VSEPR theory, a molecule with the general formula AX₃E will have a ____ molecular shape.
- a. bent
- b. trigonal planar
- c. trigonal pyramidal
- d. tetrahedral
Q. Predict the ideal bond angles around carbon in C₂I₂ using the molecular shape given by the VSEPR theory.
- a. 90°
- b. 109°
- c. 120°
- d. 180°
Q. Predict the actual bond angles in BrF₃ using the VSEPR theory.
- a. more than 120°
- b. between 109° and 120°
- c. between 90° and 109°
- d. less than 90°
Q. Which of the following has no net dipole moment?
- a. N₂O
- b. NF₃
- c. H₂Se
- d. TeO₃
Q. A molecule with the formula AX₂ uses ………. to form its bonds.
- a. sp hybrid orbitals
- b. sp² hybrid orbitals
- c. sp³ hybrid orbitals
- d. sp³d hybrid orbitals
Q. Valence bond theory predicts that carbon will use ——– hybrid orbitals in the carbonate anion, CO₃²⁻.
- a. sp
- b. sp²
- c. sp³
- d. sp³d
Q. Valence bond theory predicts that sulfur will use ——– hybrid orbitals in sulfur dioxide, SO₂.
- a. sp
- b. sp²
- c. sp³
- d. sp³d
Q. Which one of the following statements about orbital hybridization is incorrect?
- a. The carbon atom in CO₂ is sp hybridized
- b. The nitrogen atom in NH₃ is sp³ hybridized.
- c. sp² hybrid orbitals are coplanar, and at 120° to each other.
- d. sp hybrid orbitals lie at 180° to each other.
Q. For which one of the following molecules is the indicated type of hybridization not appropriate for the central atom?
- a. BeCl₂ sp²
- b. SiH₄ sp³
- c. BF₃ sp²
- d. C₂H₂ sp
Q. According to molecular orbital (MO) theory, the twelve outermost electrons in the O₂ molecule are distributed as follows:
- a. 12 in bonding MOs, 0 in antibonding MOs.
- b. 10 in bonding MOs, 2 in antibonding MOs.
- c. 9 in bonding MOs, 3 in antibonding MOs.
- d. 8 in bonding MOs, 4 in antibonding MOs.
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Q. According to molecular orbital theory, what is the bond order in the O₂⁺ ion?
- a. 5.5
- b. 5
- c. 4
- d. 2.5
Q. Which of the following statements relating to molecular orbital (MO) theory is incorrect?
- a. A bonding MO is lower in energy than the two atomic orbitals from which it is formed.
- b. Combination of two 2p orbitals may result in either Л MOs.
- c. A species with a bond order of zero will be stable.
- d. In a stable molecule having an even number of electrons, all electrons must be paired.
Q. One can safely assume that the 3s- and sp- orbitals will form molecular orbitals similar to those formed when 2s- and sp-orbitals interact. According to molecular orbital theory, what will be the bond order for the Cl₂⁺ ion?
- a. 0.5
- b. 1
- c. 1.5
- d. 2
Q. All of the following are state functions except
- a. P
- b. V
- c. q
- d. H
Q. Suppose you have a balloon of given volume, V₁, containing a gas at temperature, T₁. When you place the balloon in a colder room at temperature, T₂, the balloon’s temperature starts to drop. What are the signs of the system’s q, w, and E for this process?
- a. +q, +w, +E
- b. -q, -w, +E
- c. +q, -w, -E
- d. -q, +w, -E
Q. The melting of ice at body temperature is an endothermic process:
H₂O(s) → H₂O(l) ΔH = +6.0 kJ/mol
Thus eating ice counteracts the exothermic processes of metabolizing food. How much ice (in grams) would you have to eat to counteract the energy gained by eating 28.3g of peanuts (13 kJ/g)?
- a. 78 g
- b. 110 g
- c. 370 g
- d. 1100 g
Q. All of the following statements are false except
- a. q = H at constant T; q = E at constant V
- b. q = H at constant V; q = E at constant P
- c. q = H at constant P; q = E at constant V
- d. q = H = E at constant P or at constant V
Q. ΔH° of which of the following reactions is equal to the standard enthalpy of formation of NH₃?
- a. 3H₂(g) + N₂(g) → 2NH₃(g)
- b. 2NH₃(g) → 3H₂(g) + N₂(g)
- c. ½ H₂(g) + ½ N₂(g) → NH₃(g)
- d. NH₃(g) → ½ H₂(g) + ½ N₂(g)
Q. Calculate the standard molar enthalpy of formation of CO₂(g) in the reaction:
C(g) + O₂(g) → CO₂(g)
Given the following standard enthalpy changes:
2C(s) + O₂(g) → 2CO(g), ΔH° = -221 kJ
2CO(g) + O₂(g) → 2CO₂(g), ΔH° = -566 kJ
- a. -393.5 kJ
- b. +393.5 kJ
- c. +787.0 kJ
- d. -787.0 kJ
Q. All of the following chemical reactions are endothermic except
- a. H₂O(s) → H₂O(l)
- b. 2H₂O(g) → 2H₂(g) + O₂(g)
- c. H₂O(g) → H₂O(l)
- d. Al₂O₃(l) + 2Fe(l) → 2Al(s) + Fe₂O₃(s)
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Q. All of the followings are incorrect except
- a. Hvaprizaiton < Hsublimation < Hfusion < Hcondensation
- b. Hfusion < Hcondensation < sublimation < Hvaporization
- c. Hcondensation < Hfusion < Hvaporization < Hsublimation
- d. Hcondensation < Hsublimation < Hfusion < Hvaporization
Q. An environmental chemist got an idea that two serious pollutants (CO and NO) of the automobile exhaust can be converted to less harmful gases CO₂ and N₂. The reaction is
CO(g) + NO(g) → CO₂(g) + ½ N₂(g), ΔH° = ?
The enthalpy of this reaction as calculated from the following data is
CO(g) + ½ O₂(g) → CO₂(g), ΔH° = -283 kJ/mol
CO(g) + O₂(g) → 2NO₂(g), ΔH° = 180.6 kJ/mol
- a. -102.4 kJ
- b. -322.1 kJ
- c. -373.3 kJ
- d. -400.0 kJ
Q. A chemist heated a balloon by supplying 600 J of heat. The balloon expands doing 200 J of work against the atmospheric pressure. The change in internal energy of
- a. -800 J
- b. -400 J
- c. 0 J
- d. +400 J
Q. Spontaneous reactions are those which
- a. continue to occur once started
- b. require activation energy
- c. are endothermic
- d. are exothermic
Q. All of the following processes are spontaneous except
- a. reaction of H₂ with O₂ to form H₂O
- b. combustion of natural gas
- c. neutralization of HCl by NaOH
- d. synthesis of glucose by plants
Q. Every one knows about the importance of water. Though it is abundant in nature, yet it can be produced in laboratory by the following reaction
2H₂ + O₂ → 2H₂O
If Hf is the heat of formation of H₂O and Hr is the heat of this reaction, then
- a. Hf = Hr
- b. Hr = 2Hf
- c. Hr = ½ Hf
- d. Hf = 2Hr
Q. The following table provides different types of system and their examples but in irregular manner.
| System | Example |
|---|---|
| I. Open | a. water in cork fitted titration flask |
| II. Closed | b. pigeon |
| III. Isolated | c. ice in thermos bottle |
| Which of the following is the best match of both columns? |
- a. (I, a), (II, b), (III, c)
- b. (I, b), (II, a), (III, c)
- c. (I, c), (II, a), (III, b)
- d. (I, b), (II, c), (III, a)
Q. Sublimation, vaporization, melting, and photosynthesis all are examples of
- a. chemical processes
- b. physical processes
- c. biochemical processes
- d. endothermic processes
Q. A mixture of ice and water contains 60g of ice and 60g of water. If 60J of heat energy is removed from this mixture, then some of the
- a. water will vaporize
- b. ice will sublime
- c. ice will melt
- d. water will freeze
Q. Pieces of four different metals are present on a table. These metals are Na, Al, W, and Ti. Their melting points are 98°C, 660°C, 3410°C, and 1660°C respectively. The metal having the maximum enthalpy of fusion is
- a. Ti
- b. Al
- c. W
- d. Na
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Q. At 1000°C, the equilibrium constant for the reaction of carbon monoxide and oxygen to produce carbon dioxide is very large (Kc = 1.2 x 10²²). When the reaction is at equilibrium, the:
- a. concentration of carbon dioxide will be much larger than one or both reactants
- b. concentration of carbon dioxide will be much smaller than concentrations of both reactants
- c. concentration of carbon monoxide will be much larger than the concentration of carbon dioxide
- d. concentrations of both reactants must be much smaller than the concentration of carbon dioxide
Q. A cylinder contains an unknown gas “X.” When the cylinder is heated, a reddish-brown color develops. It means that the gas present in the cylinder was:
- a. NO₂
- b. N₂O
- c. N₂O₅
- d. N₂O₄
Q. A beaker contains a saturated solution of potassium perchlorate. When potassium chloride (KCl) is added to this solution, some of the potassium perchlorate is precipitated. It means that:
- a. KClO₄ is a stronger electrolyte than KCl
- b. Solubility of KClO₄ is greater than that of KCl
- c. Both KClO₄ and KCl are soluble in water to some extent
- d. KCl is a strong electrolyte as compared with KClO₄
Q. In salt analysis, 3rd group basic radicals (Al³⁺, Fe³⁺, etc.) are detected by adding NH₄Cl to the salt solution and then NH₄OH. 3rd group radicals are precipitated as hydroxides. In this process:
- a. NH₄Cl will ionize to a lesser extent in the presence of NH₄OH
- b. NH₄Cl will precipitate
- c. NH₄Cl will react with NH₄OH
- d. Al³⁺ will precipitate as AlCl₃
Q. If a salt is prepared by the neutralization reaction of a weak acid and a weak base, and the pKa value for the acid is greater than the pKb value for the base, then the salt prepared will be:
- a. soluble in water
- b. insoluble in water
- c. acidic
- d. basic
Q. The equivalent weight of sulfuric acid is 49. Thus, 1N solution of sulfuric acid will contain:
- a. 98g of H₂SO₄ in 1 liter of solution
- b. 49g of H₂SO₄ in 1 kg of solvent
- c. 49g of H₂SO₄ in 1 liter of solvent
- d. 49g of H₂SO₄ in 1 liter of solution
Q. A 0.5 Molar solution of NaOH contains:
- a. 40g of NaOH in 1 liter of solution
- b. 20g of NaOH in 1 liter of solution
- c. 80g of NaOH in 1 liter of solution
- d. 10g of NaOH in 1 kg of solvent
Q. A 0.5 molal solution is:
- a. less concentrated than a 0.5 molar solution
- b. has the same concentration as that of a 0.5 molar solution
- c. is 0.5 times more concentrated than a 0.5 molar solution
- d. has a concentration equal to a 1 molar solution
Q. The mole fraction of water in tap water will be:
- a. equal to 1
- b. less than 1
- c. greater than 1
- d. will be somewhat equal to 2
Q. The molality of pure water is:
- a. 36
- b. 55.5
- c. 18
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Q. All of the following are postulates of Arrhenius theory of ionization except:
- a. electrolytes ionize in water to produce cations and anions
- b. ionization is a reversible process
- c. electrical conductivity of a solution of an electrolyte depends on the extent to which the electrolyte ionizes in the solution
- d. strong electrolyte ionize to a greater extent in water
Q. If “X” moles of Ag₂Cr₂O₇ are dissolved in water to produce a saturated solution, then Ksp will be:
- a. 2X²
- b. 2X³
- c. 4X³
- d. X³
Q. A salt was dissolved in water. It was found that the ionic product is greater than the solubility product. It means that the:
- a. solution is unsaturated
- b. solution is saturated
- c. solution is supersaturated
- d. we cannot predict the saturation or unsaturation of the solution for this data
Q. Enough lead chloride PbCl₂ was dissolved in water at 25°C to produce a saturated solution. The concentration of Pb²⁺ in the solution will be:
- a. Ksp3\sqrt[3]{K_{sp}}3Ksp
- b. Ksp4\sqrt[4]{K_{sp}}4Ksp
- c. Ksp23\sqrt[3]{K_{sp}^2}3Ksp2
- d. Ksp33\sqrt[3]{K_{sp}^3}3Ksp3
Q. Consider the following cell reaction:
Pb + 2Ag⁺ → Pb²⁺ + 2Ag
If a cell is made based on this equation, then:
- a. lead will act as anode and silver as cathode
- b. lead will act as cathode and silver as anode
- c. silver will act as cathode because it has a greater reduction potential
- d. lead will act as anode because it has lesser reduction potential
Q. Consider the following spontaneous reaction:
Ni²⁺ + Mn → Ni + Mn²⁺
If a voltaic cell is made based on this reaction, then the conventional representation of the cell will be:
- a. Ni, Ni²⁺ ║ Mn²⁺, Mn
- b. Mn, Mn²⁺ ║ Ni²⁺, Ni
- c. Mn²⁺, Ni ║ Ni, Ni²⁺
- d. Ni, Ni ║ Mn, Mn²⁺
Q. 0.05 molar H₂SO₄ solution was present in the laboratory of Islamia College. Islamian genius told his friends that the pH of this solution must be:
- a. 0.05
- b. 0.5
- c. 1
- d. 2
Q. A buffer is a solution:
- a. whose pH is constant
- b. which resists change in its pH
- c. which is strong enough to maintain its pH
- d. whose pH may or may not change during a chemical reaction
Q. Consider the following list of indicators for the next two questions:
I. Ferroin
II. Methyl red
III. Diphenyl amine
IV. Allizarian yellow
V. Bromthymol blue
In this list, acid-base indicators are:
- a. I and II
- b. II, III and V
- c. III, IV and V
- d. II, IV and V
Q. In this list, redox indicators are:
- a. I and II
- b. II and III
- c. I and V
- d. III and IV
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