The reduction of iron$($III$)$ oxide $(F{e}_2{O}_3)$ to pure iron during the first step of steelmaking,

$2F{e}_2{O}_3(s)4Fe(s)+3O_2(g)$

is driven by the high$-$temperature combustion of coke, a purified form of coal:

$C(s)+O_2(g)C{O}_2(g)$

Suppose at the temperature of a blast furnace the Gibbs free energies of formation $G_f$ of $C{O}_2$ and $F{e}_2{O}_3$ are $-415.k\frac{J}{m}ol$ and $-811.k\frac{J}{m}ol,$ respectively. Calculate the minimum mass of coke needed to produce $960.t$ of pure iron. $($One metric ton, symbol $t,$ equals $1000kg.)$

Round your answer to $2$ significant digits.