Thermochemistry. Answer, step by step please. (show work)

Question

1) 2C (s) + 2H2 (g)  1C2H4 (g) ∆H = 52.3 kJ

a. Is this exothermic or endothermic?

b. Rewrite the equation with the energy as either a reactant or a product.

c. What volume of Ethene gas can be produced when 12.5 kJ are used?

Answer 1

2C(s) + 2H₂(g) ==> C₂H₄(g) ... ∆H = 52.3kJ

a. This reaction is endothermic because the sign of ∆H is positive

b. 2C(s) + 2H₂(g) + energy ==> C₂H₄(g)

c. Assuming STP (standard temperature and pressure)...

12.5 kJ x 1 mol C₂H₄ / 52.3 kJ = 0.239 mols

0.239 mols C₂H₄ x 22.4 L / mol = 5.35 L