🤓 Based on our data, we think this question is relevant for Professor Amarante's class at SUNY.
Calculate for the number of moles using the ideal gas equation and the given conditions. Divide the calculated moles by the grams provided to determine the molar mass of the gas.
Recall that ideal gas equation:
A student adds 0.1727 g of an unknown gas to a 125-mL flask. The pressure of this gas sample is found to be 0.833 atm at 20.0 °C. Is the gas likely to be methane (CH4), nitrogen (N2), oxygen (O2), neon (Ne) or argon (Ar)?
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Our tutors have indicated that to solve this problem you will need to apply the Ideal Gas Law Molar Mass concept. If you need more Ideal Gas Law Molar Mass practice, you can also practice Ideal Gas Law Molar Mass practice problems.
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Based on our data, we think this problem is relevant for Professor Amarante's class at SUNY.