need sonnboth parts (a) The standard molar entropy of ethene is 220 J K-' mol-' (with a standard state of 1 bar). Calculatethe change in Gibbs energy that occurs if 1.75 mol of ethene is cooled from 308 K to 298 K at a1.pressure of 1.00 bar.(b) Immediately following the experiment in 1(a), the sample of ethene is compressed reversibly andisothermally until the volume of the gas is 25.0 dm. What is the change in Gibbs energy during thisprocess, assuming the gas behaves ideally?

standard molar entropy of ethene (So) = 220 J/K mol moles of ethene (n) = 1.75 mol pressure (P) = 1…

(a) The standard molar entropy of ethene is 220 J K-' mol·' (with a standard state of 1 bar). Calculate the change in Gibbs energy that occurs if 1.75 mol of ethene is cooled from 308 K to 298 K at a pressure of 1.00 bar. 1. (b) Immediately following the experiment in 1(a), the sample of ethene is compressed reversibly and isothermally until the volume of the gas is 25.0 dm³. What is the change in Gibbs energy during this process, assuming the gas behaves ideally?

(a) The standard molar entropy of ethene is 220 J K-' mol·' (with a standard state of 1 bar). Calculate the change in Gibbs energy that occurs if 1.75 mol of ethene is cooled from 308 K to 298 K at a pressure of 1.00 bar. 1. (b) Immediately following the experiment in 1(a), the sample of ethene is compressed reversibly and isothermally until the volume of the gas is 25.0 dm³. What is the change in Gibbs energy during this process, assuming the gas behaves ideally?

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Chapter1: Chemical Foundations

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Question

need sonn

both parts

(a) The standard molar entropy of ethene is 220 J K-' mol-' (with a standard state of 1 bar). Calculate
the change in Gibbs energy that occurs if 1.75 mol of ethene is cooled from 308 K to 298 K at a
1.
pressure of 1.00 bar.
(b) Immediately following the experiment in 1(a), the sample of ethene is compressed reversibly and
isothermally until the volume of the gas is 25.0 dm. What is the change in Gibbs energy during this
process, assuming the gas behaves ideally?

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