The energy needed to vaporize 1.5 kg of aluminum amounts to 16.345 GJ. The heat of vaporization for aluminum is given as ΔHvap = 294000 kJ/mol. The mass of aluminum in this case equals 1.5 kg which converts to 1500 g. We can calculate the number of moles of aluminum using the formula: Mass of aluminum/(Molar Mass of aluminum). The Molar Mass of aluminum stands at 26.98 g/mol. Using this information, Number of moles calculates to 1500/26.98, which equals 55.6 moles. The total energy required can be expressed as the product of the heat of vaporization and the number of moles of aluminum, so the energy required calculates to 294000 × 55.6, resulting in 16345441.0675 kJ or approximately 16.345 GJ.
The soccer field's length is 3.94 × 10^2 in.
Length = 100 m × (39.37 in/1 m) = 394 in = 3.94 × 10^2 in
extinction coefficient (ε) = 347 L·mol⁻¹·cm⁻¹. The chemical equation representing the reaction of chromium (Cr) with hydrochloric acid (HCl) is: 2 Cr + 6 HCl → 2 CrCl₃ + 3 H₂. To find the number of moles, we apply the formula: number of moles = mass / molar weight. For chromium, we calculate: number of moles of Cr = 0.3 × 10⁻³ (g) / 52 (g/mole), leading to number of moles of Cr = 5.77 × 10⁻⁶ moles. Examining the reaction, we observe that 2 moles of Cr yield 2 moles of CrCl₃, hence 5.77 × 10⁻⁶ moles of Cr will also produce 5.77 × 10⁻⁶ moles of CrCl₃. The molar concentration is determined by: molar concentration = number of moles / volume (L), thus molar concentration of CrCl₃ = 5.77 × 10⁻⁶ / 10 × 10⁻³, which equals 5.77 × 10⁻⁴ moles/L. To convert percent transmittance (%T) to absorbance (A), we use the equation A = 2 - log(%T). Therefore, A = 2 - log(62.5), leading to A = 0.2. The relationship defining absorbance (A) includes the extinction coefficient (ε), path length (l), and concentration (c): A = εlc, hence ε = A / lc, giving ε = 0.2 / (1 × 5.77 × 10⁻⁴), which results in ε = 0.0347 × 10⁴. Thus, the extinction coefficient is ε = 347 L·mol⁻¹·cm⁻¹.
Answer: Copper is being oxidized and acts as a reducing agent. In contrast, silver is being reduced, functioning as the oxidizing agent.
Explanation:
An oxidation reaction involves the loss of electrons by an atom. Here, the oxidation state of the atom rises.
Conversely, a reduction reaction is characterized by an atom gaining electrons, resulting in a decrease in its oxidation state.
Oxidizing agents are those that facilitate the oxidation of another substance while themselves being reduced. These substances participate in reduction reactions.
Reducing agentsare defined as those that reduce other substances while undergoing oxidation themselves. They also take part in reduction reactions.
In the provided chemical reaction:
The associated half-reactions for the above process are:
Oxidation half reaction: 
Reduction half reaction: 
From the reactions outlined, copper is losing electrons. Consequently, it is oxidized and regarded as a reducing agent.
Silver is acquiring electrons, thus it is being reduced and viewed as an oxidizing agent.
