A 7.00 L tank at -8.7 °C is filled with 2.51 g of dinitrogen difluoride gas and 15.6 g of dinitrogen monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits. gas mole fraction dinitrogen difluoride dinitrogen monoxide

A 755 mL sample of gas which contains 0.0588 moles kept at 450. K would be under what pressure?

If Ar with a partial pressure of 742.4 torr is mixed with He with a partial pressure of 6.06 torr, the total pressure according to your calculator would be 748.46 torr.  The best answer, according to the rules for significant figures, would be:

If pressure and temperature remain constant, the volume of a gas increases with increasing number of gas particles.   True False

Scientists agreed upon a standard temperature and pressure (STP) to study the properties of gases at to be consistent amongst their measurements. Temperature is C (or 273K) and pressure is 1.00 atm. Use the ideal gas law to determine the volume of one mole of any gas at STP (the molar volume).

A mixture of gases contain 2.01 g of element A and 2.01 g of element B. Element A has a molar mass of 12.1 g/mol. Element B has a molar mass of 52.1 g/mol. What is the mole fraction of element B? • Report with the correct number of significant figures. • Include the correct unit. Your Answer: Answer units

In daltons and henrys law, why does the percentage of gasses in the air not decrease but the partial pressure does?

A gas with a volume of 0.553 L is initially at an unknown temperature.  The gas is submerged in boiling water (100oC) and is determined to occupy a volume of 0.247 L at constant pressure and composition.  What was the initial temperature of the gas in K?

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