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ChemBench
How much did disorder increase?
ΔS = q/T reflects that the same amount of heat causes a bigger entropy change at low temperature than at high temperature — disorder increases more dramatically when energy is added to an already-cold, more ordered system.
Entropy is the quantity behind the second law of thermodynamics — in an isolated system, total entropy only increases, which is part of why time has a direction and why some processes (like an egg unscrambling) never happen spontaneously.
Molar mass of any chemical formula (e.g. H2O, C6H12O6, Ca(OH)2).
OpenPercent composition of an element within a chemical formula.
OpenSimplest whole-number ratio formula from elemental masses or percentages.
OpenPercent yield from actual and theoretical reaction yields.
OpenEntropy change
16.779 J/K
What you entered
ΔS = q ÷ T
5000 ÷ 298= 16.7785 J/KResult
Entropy change: 16.779 J/K
ΔS for this process is 16.779 J/K.