Molar Mass Of Butane Experiment: where you put a lighter under water and release

Question

Molar Mass Of Butane Experiment: where you put a lighter under water and release it's gas into a graduated cylinder and measure out the pressure...

1. What are two major sources for error in the experiment design? If you were to do the experiment again, how would you change the experiment to reduce those two errors?

2. How many moles of argon are present in 56.2 L of argon under the conditions of standard temperature and pressure (273.0 K; 1.00 atm)? In the case, it is convenient to use the gas constant of 0.08206 L atm mol^-1K^-1.

Explanation / Answer

1. The two major sources of error maybe the amount of soap water to butane ratio and escape of gas into the atmosphere. So mostly check the mole ratio before doing the experiment and a use a pump to reduce the escape of gas.

2. use PV=nRT

P= 1atm

V= 56.2L

T=273K

therefore n= 2.508 moles

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