Reference no: EM132651054

SOLVE ACC TO NOTATION WITH PROPER DECIMAL PLACES

1. What is the molar mass (in g mol-1) of a gas which has a density of 2.06 g/L at a pressure of 1.19 bar and temperature 24.9 °C? NOTE: Your answer may not correspond to an actual gas.
2. A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.349 mol of NO2 and an unknown amount of Ne. If the partial pressure of Ne is 0.27 bar and the total pressure in the flask is 1.06 bar, calculate the mass of Ne in the flask (in g). TIP: You don't need the volume of the flask nor the temperature to solve this problem.
3. A sample of hydrogen (H2) gas was collected over water at 60°C. If the total volume of gas collected was 76.8 mL and the atmospheric pressure was 0.96 bar, what mass (in g) of hydrogen gas was collected above the water? The vapour pressure of water at 60°C is 150 torr.
4. The Haber process is used to synthesize ammonia (NH3) on a large scale by the reaction of nitrogen gas with hydrogen gas as follows: N2 (g)  + 3 H2 (g)  → 2 NH3 (g) Consider a reaction between a 9.52 L flask containing nitrogen gas and a 13.5 L flask of hydrogen gas. Both gases have a temperature of 281 K and the pressures inside both flasks is 0.85 bar. What mass of ammonia (in g) would you expect to be produced at temperature 281 K and a pressure of 0.85 bar? 
5. What is the root mean square velocity of a hypothetical gas (in m/s) which has molecular weight 59.9 g mol-1 at a temperature of 35.5 °C?