2H+ + 2e- ? H2 n=2 (# of e- involved) 8. How long must a current of 0.25 A pass through a sulfuric acid solution to liberate 0.400 L of H2 gas at STP? H2 ; n = PV / RT = (1 atm / 0.400 L) / (0.0821 LĀ·atm / KĀ·mol ? 273 K) = 0.0179 mol
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4 L of H2 gas at STP. Given that 1 mole of H2 gas at STP is equal to 22.4 L, we can calculate the charge required as follows: \[ \text{Charge} = 0.4 \, \text{L} \times \frac{1 \, \text{mol}}{22.4 \, \text{L}} = 0.017857 \, \text{mol} \] Show moreā¦
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