Gas Stoichiometry: Calculate Volume of Wet Acetylene

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AI Thread Summary
The discussion focuses on calculating the volume of wet acetylene gas produced from the reaction of calcium carbide with water. The reaction produces acetylene gas, and the user has determined the moles of dry C2H2 but is uncertain about incorporating vapor pressure into the calculation. The total pressure of the system is given as 715 torr, with the vapor pressure of water at 23.8 torr, leading to a calculated partial pressure for acetylene of 691.2 torr. The user seeks clarification on how to use these values in the ideal gas law equation, PV = nRT, to find the volume of acetylene. Understanding the relationship between total pressure, partial pressures, and the ideal gas law is essential for solving the problem.
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Homework Statement



Calcium carbide reacts with water to produce acetylene gas: CaC2 (s) + 2H2O (l) >> Ca(OH)2 (aq) + C2H2 (g). What volume of wet acetylene is collected at 25C and 715 torr when 5.20g CaC2 is reacted with an excess of water? (Vapor pressure of water at 25C = 23.8 torr)



Homework Equations



PV=nRT
P(total)=P1+P2...etc


The Attempt at a Solution



I found the moles of "dry" C2H2 (.0811 mol). However, I'm not very sure where vapor pressure and the "wet" comes in...
 
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What is the total pressure, Ptotal, of the system? What are the partial pressures?
 
Ptotal=715 torr
PH2O=23.8 torr
PC2H2=691.2 torr

I'm still not exactly sure how all of these fit in...
 
What is volume of acetylene calculated using its partial pressure?

--
methods
 
Using the equation PV = nRT, do you recall what P, V, n, R and T stand for? They also need to be in certain units. This may or may not require converting. Do you still need help for this?
 
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