Mass Balance Question:

A chlor$-$alkali plant has the following input and output streams:

INPUT $($W$1)$: an aqueous solution containing $26\%$ w$/$w of NaCl,

OUTPUT $1$: gaseous Cl$2,$ subsequently liquified $($assume pure$),$

OUTPUT $2($W$2)$: alkali product containing $50\%$ w$/$w NaOH, $1\%$ w$/$w NaCl and $49\%$ w$/$w H$2$O$,$

OUTPUT $3($W$3)$: gaseous H$2($assume pure$),$

OUTPUT $4($W$4)$: surplus water $($assume pure H$2$O$)$ from evaporator.

The plant produces $650$ tonnes of Cl$2$ per day through output $1.$

What I've worked out so far:

Balanced equation: $2$ NaCl $+2$ H$2$O $->2$ NaOH $+$ Cl$2+$ H$2$

$1.$ Number of moles of Cl$2$ in $650$ tonnes $=9\mathrm{.}155$x$10^6$ moles

$2.$ Number of moles of H$2$ in $650$ tonnes $=9\mathrm{.}155$x$10^6$ moles

$3.$ Mass of H$2$ produced per day $=18\mathrm{.}31$ tonnes$/$day

$4.$ Number of moles of NaOH in $650$ tonnes $=18\mathrm{.}31$x$10^6$ moles

$5.$ Mass of NaOH produced per day $=732\mathrm{.}4$ tonnes$/$day$.$

Can you please provide guidance on how to calculate:

$6.$ Mass of NaCl consumed per day, $($Answer is $1071\mathrm{.}1$ tonnes$/$day$)$

$7.$ Mass of H$2$O consumed per day, $($Answer is $329\mathrm{.}6$ tonnes$/$day$)$

$8.$ The mass flow in Output $2($W$2),($Answer is $1464\mathrm{.}8$ tonnes$/$day$)$

$9.$ The mass flow in Output $1($W$1),($Answer is $4176\mathrm{.}0$ tonnes$/$day$)$

$10.$ The mass flow in Output $4($W$4),($Answer is $2042\mathrm{.}9$ tonnes$/$day$)$