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An experiment shows that a 106-mL gas sample has a mass of 0.156 g at a pressure of 735 mmHg and a temp....?
An experiment shows that a 106-mL gas sample has a mass of 0.156 g at a pressure of 735 mmHg and a temperature of 31.0°C. What is the molar mass of the gas?
help :(
2 Answers
- blackbeauty14Lv 59 years agoFavorite Answer
Just slightly modify the ideal gas equation using the relationship n = mass/mol wt
PV = (m?MW)RT, convert the P to atm, 735/760 = 0.967atm, T to K 273 + 31 = 304 K and V = 0.106 L
n = 0.156/MW = 0.967*0.106/(0.0821*304) = 4.107 x 10^-3
or MW = 0.156 / 4.107 x 10^-3 = 37.98 or ~ 38 g
There you have it.
- Anonymous4 years ago
PV = nRT provide you the variety of moles of the gas, and because you have the grams, you will get the molecular mass. make certain to apply the right instruments. you will could perform a little conversions.
