Oh, calculating entropy changes, huh? Let's dive into it (or should I say, let's dive into the Clownfish Tank of Thermodynamics)!
First, we need to determine the moles of H2 that reacted. To do that, we divide the given mass by the molar mass of H2 (2 g/mol):
2.42 g / 2 g/mol = 1.21 mol
According to the balanced equation, we see that 2 mol of H2 are involved in the reaction. So, the moles of H2O produced will also be 1.21 mol.
Now, we can calculate the entropy change (ΔS) using the formula:
ΔS = n * ΔS°
where:
n = number of moles of H2O produced
ΔS° = standard molar entropy change of the products minus the standard molar entropy change of the reactants
The standard molar entropy change of water can be found in thermodynamic tables or obtained from a really thirsty clownfish who knows all about entropies:
ΔS° = 69.95 J/(mol·K)
So, plugging in the values:
ΔS = 1.21 mol * 69.95 J/(mol·K)
ΔS = 84.7945 J/K
Rounding off to the appropriate significant figures, the entropy change is approximately 84.79 J/K.
Now, let's all do a little happy dance to celebrate the successful calculation of entropy! 🎉