OBJECTIVE 1 — SELECT THE REACTION
Agent — Tomović is running out of time inside Siyahbalina Prison, and ITE gets one delivery. One dose. The antidote candidate is Prussian blue: its crystal cavities trap Tl⁺, but only small crystals expose enough surface area to trap it fast enough.
Three synthesis routes can produce Prussian blue. Before anything touches a bench, you will identify the route with the strongest thermodynamic driving force — the reaction most likely to nucleate many small crystals instead of a few large ones.
I have compiled ΔH, ΔS, and T for each candidate in Table 1. This terminal is your field notebook — run the ΔG calculations here and download the PDF report for your mission file. Report your findings through the mission memo in Canvas. Scientific evidence is our only leverage.
Rodney — ITE Field Analyst
Step 1 — Calculate ΔG for each reaction
Here is how to work the calculation, using practice data that is not one of the candidate reactions. Suppose a synthesis has ΔH = −100.0 kJ/mol, ΔS = −0.020 kJ/(mol·K), and T = 298 K:
ΔG = −100.0 − (298 × −0.020)
ΔG = −100.0 + 5.96
ΔG = −94.0 kJ/mol (rounded to the nearest tenth)
You can enter the result either way in the ΔG cell:
=, just
like Sheets or Excel — e.g. =-100.0-(298*-0.020) — then press Enter and the
calculated value takes its placeOption 2 — manual: calculate it yourself and type the answer — e.g.
-94.0
Work each candidate reaction in Table 1 the same way, using that row's ΔH, ΔS, and T values.
ΔH, ΔS, and T are given. Do the math for ΔG = ΔH − TΔS with the numbers from
each row: type a formula that starts with =, or enter your calculated value.
When you answer in Canvas, round each ΔG to the nearest tenth.
| Reaction | ΔH (kJ/mol) | ΔS (kJ/mol·K) | T (K) | ΔG (kJ/mol) |
|---|---|---|---|---|
| 1 | −85.0 | −0.050 | 298.0 | |
| 2 | −62.0 | −0.060 | 298.0 | |
| 3 | −48.0 | −0.040 | 298.0 |