Increasing the wavelength decreases the frequency of the light, which reduces the energy of the incident photons, thus decreasing the kinetic energy of emitted electrons.

The kinetic energy of the emitted electron is equal to the energy of the incident photon minus the work function of the metal.

The frequency of light must be above a certain threshold to emit electrons, but once that is achieved, the photoelectric current depends on the intensity, not the frequency.

The discriminant is zero, indicating that the roots are real and equal.

Zinc (Zn) is oxidized to Zn2+, so its oxidation state is +2.

Zinc (Zn) is oxidized to Zn2+.

Ag+ is reduced as it gains electrons to form Ag.

In this reaction, zinc (Zn) is oxidized as it loses electrons to form Zn^2+.

In AgNO3, silver has an oxidation state of +1.

Zinc is oxidized from an oxidation state of 0 to +2.

In this reaction, Ag⁺ gains electrons to form Ag, thus it is reduced.

Cr2O7^2- is reduced to Cr^3+, making it the oxidizing agent.

4 moles of Fe produce 4 moles of FeCl3. Mass of FeCl3 = 4 moles * 162.5 g/mole = 650 g.

10 g of Fe = 0.18 moles. 2 moles of Fe produce 2 moles of FeCl3. 0.18 moles of FeCl3 = 0.18 * 162.5 g = 29.25 g.

4 g of Fe = 0.071 moles. 0.071 moles of Fe produce 0.071 * 2 = 0.142 moles of FeCl3 = 0.142 * 162.5 g = 23 g.

According to the stoichiometry, 2 moles of Fe require 3 moles of Cl2. Therefore, 4 moles of Fe will require 6 moles of Cl2.

From 2 moles of Fe, 2 moles of FeCl3 are produced. Therefore, from 4 moles of Fe, 4 moles of FeCl3 are produced.

Iron (Fe) is oxidized as it loses electrons to form FeCl3.

Carbon (C) is being oxidized to carbon dioxide (CO2).

Fe2O3 is being reduced to Fe as it gains electrons.

Fe2O3 is reduced to Fe, as it gains electrons during the reaction.

Carbon is oxidized as it loses electrons to form CO2.

In this reaction, carbon (C) is oxidized as it loses electrons to form CO2.

I^- donates electrons to Fe^3+, thus it is the reducing agent.

In this reaction, Fe²⁺ is being reduced as it gains electrons to form Fe.

Iron changes its oxidation state from +2 to +3, indicating that it is oxidized.

In this reaction, Fe²⁺ is being oxidized to Fe³⁺ as it loses electrons.

Iron (Fe) is oxidized from +2 to +3 oxidation state in this reaction.

4 g of H2 = 2 moles. 1 mole of O2 is needed for 2 moles of H2, so 1 mole of O2 = 32 g is required.

First, calculate moles of H2: 4 g / 2 g/mol = 2 moles. From the reaction, 2 moles of H2 require 1 mole of O2. Therefore, 2 moles of O2 = 32 g.