the electrolysis of water, is generated at the cathode according to the half-reaction represented above. In a certain experiment, water was electrolyzed for 600 . seconds using a steady electric current. The volume of dry produced during the experiment

$2 \mathrm{H}_{2} \mathrm{O}(l)+2 e^{-} \rightarrow \mathrm{H}_{2}(g)+2 \mathrm{OH}^{-}(a q)$\nDuring the electrolysis of water, $\mathrm{H}_{2}(\mathrm{~g})$ is generated at the cathode according to the half-reaction represented above. In a certain experiment, water was electrolyzed for 600 . seconds using a steady electric current. The volume of dry $\mathbf{H}_{2}(\mathbf{g})$ produced during the experiment was 0.291 L at 298 K and 1.00 atm . \nCalculate the current, in amperes, that passed through the electrolysis cell.\nWrite your answer using three significant figures. $\square$