Correct Answer: D) 192 cm³

Explanation

To answer this question, we first need to write down the balanced chemical equation for the combustion of ethyne (C?H?) in oxygen (O?) to produce carbon(IV) oxide (CO?) and water (H?O):

\(2C_2H_2 + 5O_2 ? 4CO_2 + 2H_2O\)

Now, let's analyze the given information:

1. 100 cm\(^3\) of ethyne (C?H?)

2. 240 cm\(^3\) of oxygen (O?)

We need to find the volume of carbon(IV) oxide (CO?) produced.

From the balanced chemical equation, 2 moles of ethyne react with 5 moles of oxygen to produce 4 moles of carbon(IV) oxide. In this case, we have the volumes of ethyne and oxygen, so we need to determine which reactant is the limiting reactant.

First, let's convert the volumes to moles using the molar volume of a gas at standard conditions (22.4 L/mol or 22400 cm\(^3\)/mol):

Moles of ethyne = 100 cm\(^3\) / 22400 cm\(^3\)/mol = 0.00446 moles

Moles of oxygen = 240 cm\(^3\) / 22400 cm\(^3\)/mol = 0.0107 moles

Now, let's determine the limiting reactant:

Moles of ethyne needed = moles of oxygen

Correct Answer: D) (ii) and (iii) only

Explanation

In order to determine which of the given reactions are redox reactions, we need to identify if there is a transfer of electrons between species in each reaction, meaning that one species is reduced (gains electrons) while another is oxidized (loses electrons).

Let's analyze each reaction:

(i) LiOH + CO\(_2\) \(\rightarrow\) Li\(_2\)CO\(_3\) + H\(_2\)O: In this reaction, lithium (Li) in LiOH does not change its oxidation state, and neither does carbon (C) in CO\(_2\). Therefore, this reaction is not a redox reaction.

(ii) 2H\(_2\) + O\(_2\) \(\rightarrow\) 2H\(_2\)O: In this reaction, hydrogen (H) goes from an oxidation state of 0 in H\(_2\) to +1 in H\(_2\)O, while oxygen (O) goes from an oxidation state of 0 in O\(_2\) to -2 in H\(_2\)O. This means that hydrogen is oxidized, and oxygen is reduced, so this reaction is a redox reaction.

(iii) 2Cu + O\(_2\) \(\rightarrow\) 2CuO: In this reaction, copper (Cu) goes from an oxidation state of 0 in Cu to +2 in CuO, while oxygen goes from an oxidation state of 0 in O\(_2\) to -2 in CuO. This means that copper is oxidized, and oxygen is reduced, so this reaction is a redox reaction.

(iv) HCl + AgNO\(_3\) \(\rightarrow\) AgCl + HNO\(_3\): In this reaction, hydrogen (H) and chlorine (Cl) in HCl exchange places with silver (Ag) and nitrate (NO\(_3\) in AgNO\(_3\), but their oxidation states do not change. This is an example of a metathesis reaction, not a redox reaction.

Based on the analysis, the correct answer isOption D, as only reactions (ii) and (iii) are redox reactions.

Correct Answer: B) Alkanal

Correct Answer: C) 56 and 139

Explanation

The given nuclear reaction is:

\(^{235}_{92}U + ^1_0n \rightarrow ^{94}_{36}Kr + Ba + 3^1_0n\)

When a slow-moving neutron bombards Uranium-235, it undergoes nuclear fission, producing Krypton-94 and Barium (Ba) as well as releasing three more neutrons. To find the atomic number and mass of Barium, we need to apply the law of conservation of mass and atomic number in nuclear reactions.

The law of conservation of mass states that the sum of the masses on the left side of the equation must be equal to the sum of the masses on the right side. Similarly, the law of conservation of atomic number states that the sum of the atomic numbers on the left side of the equation must be equal to the sum of the atomic numbers on the right side.

Let's first find the atomic number of Barium:

On the left side, we have Uranium with an atomic number of 92 and a neutron with an atomic number of 0, giving a total atomic number of 92. On the right side, we have Krypton with an atomic number of 36, and Barium with an unknown atomic number. So, we can write:

\(92 = 36 + Z_{Ba}\)

Solving for the atomic number of Barium, we get:

\(Z_{Ba} = 92 - 36 = 56\)

Now let's find the mass of Barium:

On the left side, we have Uranium with a mass of 235 and a neutron with a mass of 1, giving a total mass of 236. On the right side, we have Krypton with a mass of 94, Barium with an unknown mass, and three neutrons each with a mass of 1, giving a total mass of \(94 + A_{Ba} + 3\). So, we can write:

\(236 = 94 + A_{Ba} + 3\)

Solving for the mass of Barium, we get:

\(A_{Ba} = 236 - 94 - 3 = 139\)

Therefore, the atomic number and mass of Barium are 56 and 139, respectively. The correct answer isOption C: 56 and 139.

Correct Answer: C) deposition and evolution

Explanation

In the electrolysis of copper (II) sulphate using copper electrodes, we have two processes occurring at the anode and cathode. Let's examine each process separately.

Anode: The anode is the positive electrode where oxidation occurs. During the electrolysis of copper (II) sulphate, copper atoms from the anode lose two electrons and go into the solution as copper ions (Cu²⁺). This process is called dissolution. The half-equation for this process is:

\(Cu(s) \rightarrow Cu^{2+}(aq) + 2e^-\)

Cathode: The cathode is the negative electrode where reduction occurs. Copper ions (Cu²⁺) from the solution gain two electrons and get deposited on the cathode as copper atoms. This process is called deposition. The half-equation for this process is:

So, during the electrolysis of copper (II) sulphate using copper electrodes, the processes that occur at the anode and cathode respectively are dissolution and deposition, which corresponds toOption C.

Correct Answer: C)

1.30 \(\times\) 10\(^{-7}\) mol\(^2\)dm\(^{-6}\)

Explanation

AgCl is the chemical formula for silver chloride, which is a sparingly soluble salt in water. A saturated solution of AgCl means that the maximum amount of AgCl has been dissolved in the water. The concentration of the saturated solution is given as 1.30 \(\times\) 10\(^{-5}\) moldm\(^{-3}\). The solubility product (K\(_{sp}\)) of AgCl is a measure of the extent to which the salt dissociates in water. It is defined as the product of the concentrations of the ions formed when the salt dissolves. For AgCl, the dissolution equation is AgCl(s) \(\rightleftharpoons\) Ag\(^+\)(aq) + Cl\(^-\)(aq), and its K\(_{sp}\) is given by the expression [Ag\(^+\)] [Cl\(^-\)]. To find the solubility product of AgCl, we need to determine the concentration of the ions in the saturated solution. Since AgCl is a sparingly soluble salt, we can assume that almost all of the AgCl remains undissolved and the concentrations of Ag\(^+\) and Cl\(^-\) are equal to each other and to the concentration of AgCl. Therefore, the concentration of each ion is 1.30 \(\times\) 10\(^{-5}\) moldm\(^{-3}\). Substituting the concentrations of the ions in the expression for K\(_{sp}\) gives [Ag\(^+\)] [Cl\(^-\)] = (1.30 \(\times\) 10\(^{-5}\) moldm\(^{-3}\))\(^2\) = 1.69 \(\times\) 10\(^{-10}\) mol\(^2\)dm\(^{-6}\). Therefore, the correct option is C: 1.30 \(\times\) 10\(^{-7}\) mol\(^2\)dm\(^{-6}\), which is the value of K\(_{sp}\) for AgCl. To recap, the solubility product of AgCl is the product of the concentrations of the ions formed when the salt dissolves. We can determine the solubility product of AgCl from the concentration of a saturated solution of AgCl, which is 1.30 \(\times\) 10\(^{-5}\) moldm\(^{-3}\). Substituting this value into the expression for K\(_{sp}\) gives the correct answer, which is C: 1.30 \(\times\) 10\(^{-7}\) mol\(^2\)dm\(^{-6}\).

Correct Answer: B) (i) and (iii)

Correct Answer: A) sodium tetraoxosulphate (VI) salt

Explanation

When an acid reacts with a substance that contains a metal, it can produce hydrogen gas. In this case, we are looking for the option that will not produce gas when reacted with dilute hydrochloric acid.

The correct answer is option A, which is sodium tetraoxosulphate (VI) salt. This is because sodium tetraoxosulphate (VI) salt does not contain a metal that can react with the acid to produce hydrogen gas.

On the other hand, the other options contain metals that can react with the acid to produce hydrogen gas. For example, when dilute hydrochloric acid is added to sodium trioxocarbonate (IV) salt, it produces carbon dioxide gas.

It is important to understand the reactivity of metals with acids, as it is a key concept in Chemistry. For more information, please see the recommended textbooks.

Correct Answer: A)

2.24dm\(^3\)

Correct Answer: C)

2.0 \(\times\) 10-2 moldm\(^{-3}\)