MCQ
Using the rules for significant figures, the correct answer for the expression $\frac{0.02858 \times 0.112}{0.5702}$ will be .... .
- A$0.005613$
- ✓$0.00561$
- C$0.0056$
- D$0.006$
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$2H_2(g) + O_2(g) \to 2H_2O(l)$ ; $\Delta _fH^o_{298}(H_2O(l)) = -285.5\, kJ/mol$
What is $\Delta S^o_{298}$ for the given fuel cell reaction ?
Given $: O_2(g) + 4H^+(aq) + 4e^- \to 2H_2O(l)$ $E^o = 1.23\, V$