What is the density of a gas at STP that has a molar mass of 50.0 g/mol?
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Answer:
Density = mass/volume Let us assume a volume of 1 L. We know that 1 mol gas = 22.4 L gas at STP, or 1 L = 0.0446 mol. We can do some dimensional analysis to figure out how many grams of the gas are in 1 L. 1 L * (0.0446 mol/1 L) * (50.0 g/1 mol) = 2.23 g Density = mass/volume = 2.23 g / 1 L = 2.23 g/L
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Other answers
"STP" is Standard Temperature and Pressure. Standard temperature is 0 ° C or 273 K. Standard pressure is 1 atmosphere or 760 mm Hg (also called "torr"). 1 mole of any gas at STP occupies 22.4 liters of volume. Therefore: 50g per mole = 50g per 22.4 liters ; now setup a ratio to figure grams (g) per liter: 50g divided by 22.4 liters = 2.23g per liter in density at STP
Tammy
Density = mass/volume Let us assume a volume of 1 L. We know that 1 mol gas = 22.4 L gas at STP, or 1 L = 0.0446 mol. We can do some dimensional analysis to figure out how many grams of the gas are in 1 L. 1 L * (0.0446 mol/1 L) * (50.0 g/1 mol) = 2.23 g Density = mass/volume = 2.23 g / 1 L = 2.23 g/L
Hellamun...
"STP" is Standard Temperature and Pressure. Standard temperature is 0 ° C or 273 K. Standard pressure is 1 atmosphere or 760 mm Hg (also called "torr"). 1 mole of any gas at STP occupies 22.4 liters of volume. Therefore: 50g per mole = 50g per 22.4 liters ; now setup a ratio to figure grams (g) per liter: 50g divided by 22.4 liters = 2.23g per liter in density at STP
Tammy
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