Test: Chemistry Minor Mock Test- 2 (March 19) - NEET MCQ

Specific conductance = Cell constant/Resistance
∴ Specific conductance ∝ 1/Resistance 
∴ The one with the lowest resistance (order 10^-9) will have the highest specific conductance.
Hence, option A is correct.

As we move along the period electronegativity increases due to increase in nuclear charge.

NaCl → Na⁺ + Cl⁻
No. of moles of Na⁺ ions = 0.025
No. of Na⁺ ions = 0.025 x 6.023 x 10²³ = 1.505 × 10²²

n = order of the reaction =slope of the line
Larger the value of the slope of the line, larger the order.
Thus, P = 3, Q = 2, R = 1, S = 0.

The reaction of metallic cobalt in a nickel sulfate solution involves a competition for the release of electrons. This means that the cobalt metal can react with the nickel ions in the solution, or the nickel can deposit on the cobalt metal.

At equilibrium, the reaction has balanced out with no net change in the concentration of the reactants and products. The fact that both Ni⁺² (aq) and Co⁺² (aq) are present at moderate concentrations at equilibrium signifies that neither forward nor reverse reactions are greatly favoured.

• A: This option is incorrect because both reactants and products are present in moderate concentrations, indicating that neither is greatly favoured.
• B: This statement is not correct either. Even though Co (s) and Ni⁺² (aq) are part of the reaction, the fact that Co⁺² (aq) is also present at moderate concentrations shows that they are not the only favoured species.
• C: This option is also incorrect. Even though Co⁺² (aq) and Ni (s) are part of the reaction, the fact that Ni⁺² (aq) is also present at moderate concentrations shows that they are not the only favoured species.
• D: This is the correct answer. When a reaction is at equilibrium, it means that the rate of the forward reaction equals the rate of the reverse reaction. Therefore, neither the reactants nor the products are greatly favoured. In other words, the concentrations of the reactants and products remain constant over time

• Oxidation Numbers of Halogens: The halogens (Fluorine, Chlorine, Bromine, Iodine, and Astatine) are a group in the periodic table. They are known for their high electronegativity and hence, when they combine with almost all other elements, they tend to have an oxidation number of -1 as they gain one electron to achieve a stable electronic configuration.
• Exception in the case of Oxygen: However, oxygen is more electronegative than all halogens except fluorine. So, when halogens (chlorine, bromine, and iodine) combine with oxygen, they tend to lose electrons to oxygen and hence, they show positive oxidation states.
• Conclusion: Therefore, when chlorine, bromine, and iodine are combined with oxygen, they have an oxidation number of +1 or any positive number (depending on the number of oxygen atoms they are combined with). Hence, the correct answer is C: +1 or any positive number.

Here, we can see that in the initiation and termination step, radical is formed.

Rate = k (A)[B]

The given reaction is first order in A and first order is B.
Thus, total order = 2

(a) Unit of k = cone ^{1 - n} time ^-1 = conc^-1 time^-1 Thus, (a) is false.
(b)  of second-order reaction, thus (b) is false. 

Thus, (c) is correct.

Thus, value of k is dependent on the concentration of A and B. Thus, (d) is false.

Carbocation is most reactive as it lacks electrons. So it need an electron to attain stability.

Fe (OH)₃ is used to remove arsenic impurities.

The three CH₃ radicals attached to the positively charged carbon are electron repelling group. Therefore, these CH₃ radicals exhibit +I effect (Inductive effect) and repel electrons towards the positively charged Carbon. This decreases the positive charge and makes the compound more stable.

F₂ is very strong oxidizing agent.

When zinc is placed in copper nitrate solution the intensity of the blue colour is produced and copper iron is deposited on zinc.

• This is a Redox reaction between zinc and an aqueous solution of copper nitrate occurring in a beaker.

The correct order of equivalent conductance at infinite dilution is KCl > NaCl > LiCl.

Anion is same (chloride ion) for all the species. Larger is the size of the cation, greater is the equivalent conductance at infinite dilution and vice versa.

No. of moles of NaOH = 10/40 = 0.25 mol

(a)

I, II, V - represent first order equation

III, VI - zeroth order equation

IV - second order equation

Mass of C₂H₅OH = 85 g
Molar mass of C₂H₅OH = 46 g/mol
nC₂H₅OH = 85/46 = 1.85 mol
Mass of water = 100 - 85 = 15 g
nH₂O = 15/18 = 0.833 mol

Mass of solute is obtained by multiplying % weight with mass of solvent and obtaining an answer divided by 100.
Mass of solute in 200g of 30% solution can be obtained as follows:
30% by weight indicates 30g of solute is present in 100g of solvent so 60g of solute will be present in 200g of solution.
20% by weight indicates 20g of solute is present in 100g of solvent so 60g of solute will be present in 300g of solution
So on mixing these both solutions, mass of solute is 60g +60g =120g
Mass of solution on mixing is 200g +300g =500g
Percent of solute can be obtained as follows:

24% percentage of solute in the final solution.

A disproportionation reaction is a particular type of redox reaction in which a single compound is transformed into two different compounds, one being reduced and the other being oxidized.

The decomposition of hydrogen peroxide to form water and oxygen is a classic example of a disproportionation reaction.

Determining Anodes when connected to the Standard Hydrogen Electrode

The Standard Hydrogen Electrode (SHE) is commonly used as a reference electrode in electrochemistry and has an electrode potential of 0V. The electrode with a lower reduction potential than the SHE will act as the anode (site of oxidation), while the electrode with a higher reduction potential than the SHE will act as the cathode (site of reduction).
A: Fe/Fe²⁺ E₀= − 0.44
The reduction potential of this electrode is lower than that of the SHE, so it will act as the anode when connected to the SHE.
B: Al/Al³⁺ E₀= - 1.66
The reduction potential of this electrode is lower than that of the SHE, so it will also act as the anode when connected to the SHE.
C: F₂(g)/2F⁻(aq) E₀= + 2.87
The reduction potential of this electrode is higher than that of the SHE, so it will act as the cathode, not the anode, when connected to the SHE.
D: Cu/Cu²⁺ E₀= + 0.34
The reduction potential of this electrode is higher than that of the SHE, so it will also act as the cathode, not the anode, when connected to the SHE.

Therefore, electrodes A: Fe/Fe²⁺ (E₀= − 0.44) and B: Al/Al³⁺ (E₀= - 1.66) will act as anodes when connected to the Standard Hydrogen Electrode.

BF₃ reacts with LiAlH₄ to form B₂H₆ which reacts with NH₃NH₃ in 1:2 ratio forming B₃N₃H₆( Borazine , inorganic benzene

Non metals have high value of ionization energy while metals have comparatively low value of ionization energy.

• Autoxidation is any oxidation that occurs in presence of oxygen.
• The term is usually used to describe the degradation of organic compounds in air (as a source of oxygen).
• Autoxidation produces hydroperoxides and cyclic organic peroxides.

Heterolytic fission, also known as heterolysis, is a type of bond fission in which a covalent bond between two chemical species is broken in an unequal manner, resulting in the bond pair of electrons being retained by one of the chemical species (while the other species does not retain any of the electrons from the bond pair). When a neutrally charged molecule undergoes heterolytic fission, one of the products will have a positive charge whereas the other product will have a negative charge.