Final answer:
The mass of NO2 in the final equilibrium mixture cannot be determined from the given options because the calculated mass of 5.15 g does not correspond with any listed choices, suggesting either a mistake in the provided information or the answer options(option d).
Step-by-step explanation:
The question is asking to determine the mass of NO2 in the equilibrium mixture resulting from the given reaction. To find this mass, we first need to understand how the equilibrium concentrations are related through the balanced chemical equation:
2NOCI(g) → 2NO(g) + Cl2(g)
Since the chemical equation shows that 2 moles of NOCI decompose to form 2 moles of NO and 1 mole of Cl2, we can use the stoichiometric relationships to determine the concentration changes. With a change in the concentration of Cl2 being Δ[Cl2] = 0.028 M, we can infer that 2 moles of NO2 are produced for every 1 mole of Cl2.
Thus, the change in NO2 concentration (Δ[NO2]) will be twice that of Cl2, resulting in a Δ[NO2] = 0.056 M in the 2.00 L container. The number of moles of NO2 is thus 0.056 M × 2.00 L = 0.112 moles. To find the mass, we use the molar mass of NO2 (46.01 g/mol):
Mass of NO2 = 0.112 moles × 46.01 g/mol = 5.15 g
However, since this result is not listed as one of the options, there may be a mistake in the information provided or the options available. Therefore, the correct answer would be D) The mass cannot be determined from the information given.