Use the following to answer the question: -The internal energy for a diatomic gas is given by U = 5nRT/2.Calculate the internal energy of a 100 g mixture of oxygen (20%)and nitrogen (80%)gas at 25 $\circ$ C.(The molar weight of O₂ = 32 g,and the molar weight of N₂ = 28 g.) A)21.6 kJ B)1.80 kJ C)12.1 kJ D)13.0 kJ E)1.10 kJ

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The internal energy of a diatomic gas is given by $U = \frac{5}{2}nRT$, where $n$ is the number of moles, $R$ is the gas constant (8.314 J/mol·K), and $T$ is the temperature in Kelvin. To find the internal energy of the mixture, we first need to calculate the number of moles of each gas and then apply the formula.1. Convert the temperature from Celsius to Kelvin: $T = 25 + 273.15 = 298.15 K$.2. Calculate the mass of each gas: Oxygen (20% of 100g) = 20g, Nitrogen (80% of 100g) = 80g.3. Calculate the moles of each gas: Moles of O2 = $20g / 32g/mol = 0.625 mol$, Moles of N2 = $80g / 28g/mol = 2.857 mol$.4. Total moles = $0.625 mol + 2.857 mol = 3.482 mol$.5. Apply the formula for internal energy: $U = \frac{5}{2} \times 3.482 mol \times 8.314 J/mol·K \times 298.15 K$.After calculating, the internal energy $U$ is approximately 21.6 kJ, making option A the correct answer.

Use the Following to Answer the Question: -The Internal ∘\circ∘

Use the Following to Answer the Question:
-The Internal $\circ$