(Solved): Consider the following reaction for the decomposition of hydrogen disulfide: 2H2S(g)<= ...

Consider the following reaction for the decomposition of hydrogen disulfide: $$2{\mathrm{H}}_2\mathrm{S}(\mathrm{g})\text{ <======> }2{\mathrm{H}}_2(\mathrm{g})+{\mathrm{S}}_2(\mathrm{g}){\mathrm{K}}_{\mathrm{c}}=1.67\times 10^{?7}\text{ at }800^{?}\mathrm{C}$$ A 2.00 L reaction vessel initially contains $$0.202\mathrm{mol}$$ of $${\mathrm{H}}_2\mathrm{S}$$ at $$800^{?}\mathrm{C}$$. A. Find the equilibrium concentration of $$\left[{\mathrm{H}}_2\mathrm{S}\right]$$ B. Find the equilibrium concentration of $$\left[{\mathrm{H}}_2\right]$$ C. Find the equilibrium concentration of $$\left[S_2\right]$$ D. Find the $$K_p$$ for the reaction at $$800^{?}\mathrm{C}$$. A A