CaC2 + H2O → C2H2 + Ca(OH)2
Ca 1 1
C 2 2
H 2 4
O 1 2
CaC2 + 2 H2O → C2H2 + Ca(OH)2
Ca 1 1
C 2 2
2 4 4
1 2 2
Balanced: CaC2 + 2 H2O → C2H2 + Ca(OH)2
= 0.2415 mol C2H2
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas, C2H2, and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC2, with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons.
(a) Outline the steps necessary to answer the following question: What volume of C2H2 at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC2 with water?
(b) Answer the question.
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