The figure shows two concentration cells at $298\ \text{K}$. Cell I is $\text{Ag}\,|\,\text{Ag}^+(0.0010\ \text{mol L}^{-1})\,\|\,\text{Ag}^+(0.100\ \text{mol L}^{-1})\,|\,\text{Ag}$, with $50.0\ \text{mL}$ of solution on each side and a salt bridge of potassium nitrate. In cell II, two hydrogen electrodes dip into the same $0.10\ \text{mol L}^{-1}$ hydrochloric acid, kept apart by a glass frit. Hydrogen is bubbled over the left electrode at $0.10\ \text{bar}$ and over the right one at $1.0\ \text{bar}$. Take $\dfrac{2.303RT}{F} = 0.059\ \text{V}$ and $F = 96487\ \text{C mol}^{-1}$, and treat the solutions as ideal. Each cell is joined only to a voltmeter at first. Which of the following statements are correct?

Fig. 1: Two concentration cells side by side. Cell I: two beakers with silver electrodes, the left solution Ag+ 0.0010 mol per litre and the right Ag+ 0.100 mol per litre, each 50.0 mL, joined by a potassium nitrate salt bridge. Cell II: one vessel of hydrochloric acid, 0.10 mol per litre, split by a glass frit, with a platinum hydrogen electrode on each side; hydrogen is bubbled at 0.10 bar on the left and at 1.0 bar on the right.