🤓 Based on our data, we think this question is relevant for Professor Marinescu's class at USC.
Since we are given a value for density and we are looking for the molar mass we use a derivative of the ideal gas law given below:
Aside from the given density (3.93 g/L), we should know that at STP, P = 1 atm and T = 273.15 K. We should also know that the ideal gas constant R = 0.08026 L•atm/mol•K.
The density of a certain gaseous fluoride of phosphorus is 3.93 g/L at STP. Calculate the molar mass of this fluoride and determine its molecular formula.
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Our tutors have indicated that to solve this problem you will need to apply the Standard Temperature and Pressure concept. You can view video lessons to learn Standard Temperature and Pressure. Or if you need more Standard Temperature and Pressure practice, you can also practice Standard Temperature and Pressure practice problems.
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Based on our data, we think this problem is relevant for Professor Marinescu's class at USC.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.