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Acetylene gas (C2H2) is produced as a result of the reaction CaC2(s) + 2 H2O(ℓ) → C2H2(g) + Ca(OH)2(aq). If 10 g of CaC2 are consumed in this reaction, how much H2O is needed? Answer in units of mol.

1 Answer

Apr 10, 2018

0.312 mol

Explanation:

First, find the number of moles of $C a C_{2}$ $CaC_2$ that is used by dividing the mass by the molar mass.

Molar mass: $40.08 + 2 (12.01) = 64.1$ $40.08+2(12.01)=64.1$ $g m o l^{- 1}$ $gmol^-1$

$\frac{10 g}{64.1 g m o l^{- 1}} = 0.156$ $(10g)/(64.1gmol^-1)=0.156$ $m o l$ $mol$ of $C a C_{2}$ $CaC_2$ reacted

From the stoichiometry, we can see that for every mol of $C a C_{2}$ $CaC_2$ , 2 mol of $H_{2} O$ $H_2O$ is needed

$2 \times 0.156 = 0.312$ $2 xx 0.156=0.312$ $m o l$ $mol$ of $H_{2} O$ $H_2O$

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