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One mole of an ideal gas is subjected to a change from 10 atm to 1 atm at 300 K. Calculate (in JK-1 rounded up to three decimal places) ∆Ssurrounding = ? [R = 8.314 JK-1mol-1]
    Correct answer is '-8.314'. Can you explain this answer?
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    One mole of an ideal gas is subjected to a change from 10 atm to 1 atm...
    Explanation:

    To calculate the change in entropy of the surroundings (Ssurrounding), we can use the equation:

    Ssurrounding = -ΔH/T

    where ΔH is the enthalpy change and T is the temperature.

    Step 1: Calculate the enthalpy change (ΔH)
    We can calculate the enthalpy change using the ideal gas equation:

    ΔH = ΔnRT

    where Δn is the change in the number of moles, R is the gas constant, and T is the temperature.

    In this case, since we have one mole of gas, the change in the number of moles is 1.

    ΔH = (1 mol)(8.314 JK-1mol-1)(300 K)
    = 2494.2 J

    Step 2: Calculate the change in entropy of the surroundings (Ssurrounding)
    Now we can substitute the values into the equation for Ssurrounding:

    Ssurrounding = -ΔH/T
    = -(2494.2 J)/(300 K)
    ≈ -8.314 JK-1

    Final answer:
    The change in entropy of the surroundings (Ssurrounding) is approximately -8.314 JK-1.
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    One mole of an ideal gas is subjected to a change from 10 atm to 1 atm at 300 K. Calculate (in JK-1 rounded up to three decimal places) ∆Ssurrounding = ? [R = 8.314 JK-1mol-1]Correct answer is '-8.314'. Can you explain this answer?
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