(a) Balance the equation.
b) Calculate the mol CS2 produced when 1.13 mol S8 is used.
(c) How many mol H2S is produced?
CH4(g) + S8(s) --> CS2(l) + H2S(g)
a) 2 CH4(g) + S8(s) --> 2 CS2(l) + 4 H2S(g)
b) Since 1 mol of S8(s) produces 2 moles of CS2(l)
1.13 moles of S8 x 2 moles of CS2 = 2.26 moles of CS2(l) produced
c) 4 moles of H2S(g) is produced
2[CH4](g) + [S8](s) ---> 2[CS2](l] + 4[H2S](g)?
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CH4(g) + S8(s) --> CS2(l) + H2S(g)
a) 2 CH4(g) + S8(s) --> 2 CS2(l) + 4 H2S(g)
b) Since 1 mol of S8(s) produces 2 moles of CS2(l)
1.13 moles of S8 x 2 moles of CS2 = 2.26 moles of CS2(l) produced
c) 4 moles of H2S(g) is produced
2[CH4](g) + [S8](s) ---> 2[CS2](l] + 4[H2S](g)?