How many grams of $CO_2$ and grams of $H_2O$ are produced when 52.0 g $C_2H_2$ burns in oxygen?

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Answer 1 · 2016-05-20T18:38:13

$H-C-=C-H(g) + 5/2O_2(g) rarr 2CO_2(g) + H_2O$

$H-C-=C-H(g) + 5/2O_2(g) rarr 2CO_2(g) + H_2O(l)$

$"Moles of acetylene"$ $=$ $(52.0*g)/(26.04*g*mol^-1)$ $=$ $2*mol$

Given the molar equivalence, $4*molxx44.0*g*mol^-1$ $CO_2$ are produced, as well as $36.0*g$ water.

How many grams of CO_2CO_2 and grams of H_2OH_2O are produced when 52.0 g C_2H_2C_2H_2 burns in oxygen?