Question 7 (Should you need a copy of the Periodic Table for this question, you will find one on page 8 of this document.) Calculations using Boyle's Law a) 5.00L of

a gas is at 1.08atm. What pressure is obtained when the volume is 10.0L? b) 9.48L of a gas was at an unknown pressure. However, at standard pressure, its volume was measured to be 8.00L. What was the unknown pressure? Calculations using Charles' Law c) A gas is collected and found to fill 2.85L at 25.0°C. What will be its volume at standard temperature? d) 5.00L of a gas is collected at 100K and then allowed to expand to 20.0L. What must the new temperature be in order to maintain the same pressure? Calculations using Gay-Lussac's Law e) 10.0L of a gas is found to exert 97.0kPa at 25.0°C. What would be the required temperature (in Celsius) to change the pressure to standard pressure? f) 5.00L of a gas is collected at 22.0°C and 745.0mmHg. When the temperature is changed to standard, what is the new pressure? Calculations using The Combined Gas Law Remember, that STP is a common abbreviation for "standard temperature and pressure". g) 2.00L of a gas is collected at 25.0°C and 745.0mmHg. What is the volume at STP? h) The pressure of 8.40L of nitrogen gas in a flexible container is decreased to one-half its original pressure, and its absolute temperature is increased to double the original temperature. What is the new volume? Calculations using Avogadro's Law i) 5.00L of a gas is known to contain 0.965mol. If the amount of gas is increased to 1.80mol, what new volume will result (at an unchanged temperature and pressure)? i) A cylinder with a movable piston contains 2.00g of helium (He), at room temperature. More helium was added to the cylinder and the volume was adjusted so that the gas pressure remained the same. How many grams of helium were added to the cylinder if the volume was changed from 2.00L to 2.70L? (The temperature was held constant.) Calculations using The Ideal Gas Law k) A sample of dry gas weighing 2.1025g is found to occupy 2.850L at 22.00°C and 740.0mmHg. How many moles of the gas are present? 1) At STP, a 5.00L flask filled with air has a mass of 543.251g. The air in the flask is replaced with another gas and the mass of the flask is 566.107g. The density of air is 1.29g/L. What is the gas that replaced the air?