Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2, and oxygen gas, O2 to produce the following combustion reaction:
2C2H2(g)+5O2(g)→4CO2(g)+2H2O(g)
Imagine that you have a 5.00 L gas tank and a 2.50 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 155 atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases.
CHEM HELP?
2017-10-12 12:19 am
回答 (2)
2017-10-12 1:00 am
✔ 最佳答案
Gas law: PV = nRTO₂ tank: P₁ = 155 atm, V₁ = 5.00 L
C₂H₂ tank: P₂ = ? atm, V₂ = 2.50 L
2C₂H₂(g)+5O₂(g)→4CO₂(g)+2H₂O(g)
Mole ratio n₂/n₁ = 2/5
At constant temperature: PV/n = RT = constant
Hence, P₁V₁/n₁ = P₂V₂/n₂
Pressure of C₂H₂ tank, P₂
= P₁ × (V₁/V₂) × (n₂/n₁)
= (155 atm) × (5.00/2.50) × (2/5)
= 124 atm
2017-10-12 12:21 am
Not important because I have 5 spare tanks of each in the shed outside.
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