The Battle for Chemical Domination On the Open Seas Group Slaughter The Battle for Chemical Domination On the Open Seas

Set-Up: Number 1-10 on your piece of paper. Each team member must print their name next to ONE number only. Don’t let any other team see what your numbers are! These are your battleships. If your team has less than 4 members, add sufficient names to reach 4 total people.

The Rules You gain the ability to take shots at other teams’ battleships by getting questions correct. Questions are worth 1, 2, or 3 shots at the team of your choice. When one of your battleships is sunk, the person who’s battleship was shot will be rescued by their teammates. THE TEAM ONLY DIES WHEN EVERY MEMBER HAS BEEN SHOT. Once a team is dead, if they get the next question right, they will come back to life as angry ghosts! Ghosts get double shots for every question they get right.

The Rules: Part II Winners will be determined by which team has the most LIVING battleships at the end of the class. All students MUST participate. You show this by making sure everyone’s color appears in the answer. Sharing pens results in immediate disqualification for that question. Answers are only accepted if written on the group’s white board! NO FRIENDLY FIRE ;)

May the odds be ever in your favor… Last Questions? Let the games begin! May the odds be ever in your favor…

Question 1: for 2 shots 1 The volume of a gas at 99.0 kPa is 300.0 mL. If the pressure is increased to 188 kPa, what will be the new volume in milliliters? Draw a graph to represent the relationship between pressure and volume

Question 1: for 2 shots The volume of a gas at 99.0 kPa is 300.0 mL. If the pressure is increased to 188 kPa, what will be the new volume? Draw a graph to represent the relationship between pressure and volume

Question 2: for 2 shots Determine how many moles of water vapor will be produced at 1.00 atm and 200.°C by the complete combustion of 10.5 L of methane gas (CH4).

Question 2: for 2 shots Determine how many moles of water vapor will be produced at 1.00 atm and 200.°C by the complete combustion of 10.5 L of methane gas (CH4).

Question 3: for 1 shot A 2.00 L flask is filled with propane gas (C3H8) at 1.00 atm and -15.0°C. What is the mass of the propane in the flask?

Question 3: for 1 shot A 2.00 L flask is filled with propane gas (C3H8) at 1.00 atm and -15.0°C. What is the mass of the propane in the flask?

Question 4: for 1 shot An unopened, cold 2.00 L soda bottle contains 46.0 mL of gas confined at a pressure of 1.30 atm at a temperature of 5.0°C. If the bottle is dropped into a lake and sinks to a depth at which the pressure is 2.85 atm and the temperature is 2.09°C, what will be the volume (in mL) of gas in the bottle?

Question 4: for 1 shot An unopened, cold 2.00 L soda bottle contains 46.0 mL of gas confined at a pressure of 1.30 atm at a temperature of 5.0°C. If the bottle is dropped into a lake and sinks to a depth at which the pressure is 2.85 atm and the temperature is 2.09°C, what will be the volume of gas in the bottle?

Question 5: for 1 shot What is the assumption of KMT that explains why gases are highly compressible?

Question 5: for 1 shot What is the assumption of KMT that explains why gases are highly compressible? Gas particles are tiny compared to the HUGE amounts of space between them

Question 6: for 2 shots CaCO3  CaO + CO2 Carbon dioxide gas is collected over water from the decomposition of calcium carbonate. At 25oC and a barometric pressure of 755mmHg, the carbon dioxide had a volume of 842 mL. The partial pressure of water at 25oC is 23 mmHg. How many moles of CO2 were collected? How many grams of calcium carbonate were required to produce the CO2 sample?

Question 6: for 2 shots Carbon dioxide gas is collected over water from the decomposition of calcium carbonate. At 25oC and a barometric pressure of 755mmHg, the carbon dioxide had a volume of 842 mL. The partial pressure of water at 25oC is 23 mmHg. How many moles of CO2 were collected? How many grams of calcium carbonate were required to produce the CO2 sample?

Question 7: for 1 shot Three 2.0 L containers are placed in a 50.°C room. Sample of 0.5 moles of N2, 0.5 moles of Xe, and 0.5 moles of CO2 are pumped into containers 1, 2, and 3, respectively. Inside which container will the pressure be greatest? Which container has the molecules with the greatest average kinetic energy? Which container has the molecules with the greatest velocity?

Question 7: for 1 shot Three 2.0 L containers are placed in a 50.°C room. Sample of 0.5 moles of N2, 0.5 moles of Xe, and 0.5 moles of CO2 are pumped into containers 1, 2, and 3, respectively. Inside which container will the pressure be greatest? All the same! (Same V, T, n = same P; Avogadro’s Principle) Which container has the molecules with the greatest average kinetic energy? All the same! (Same temp = same average kinetic energy) Which container has the molecules with the greatest velocity? N2 (lower molar mass = greater velocity!)

Question 8: for 1 shot If we increase the pressure of a gaseous system by a factor of 4 and raise the temperature by a factor of 8, then the volume of the system will ______________ by a factor of ______.

Question 8: for 1 shot If we increase the pressure of a gaseous system by a factor of 4 and raise the temperature by a factor of 8, then the volume of the system will increase by a factor of 2.

Question 9: for 1 shot The lowest pressure achieved in a laboratory is about 1.0x10-15 mmHg. How many molecules of gas are present in a 1.00 L sample at that pressure and a temperature of 22.0°C?

Question 9: for 1 shot The lowest pressure achieved in a laboratory is about 1.0x10-15 mmHg. How many molecules of gas are present in a 1.00 L sample at that pressure and a temperature of 22.0°C?

Question 10: for 1 shot Each of these flasks is the same size and at the same temperature. Which one contains the most molecules?

Question 10: for 1 shot Each of these flasks is the same size and at the same temperature. Which one contains the most molecules? Flask 4 contains the most molecules because it is at the highest pressure! V and T are constant so we are looking at the direct relationship between P and n.

Question 11: for 1 shot The Celsius temperature of a 3.00 L sample of gas is lowered from 80.0°C to 30.0°C. What will be the resulting volume of this gas? Draw a graph to represent the relationship between temperature and volume

Question 11: for 1 shot The Celsius temperature of a 3.00 L sample of gas is lowered from 80.0°C to 30.0°C. What will be the resulting volume of this gas? Draw a graph to represent the relationship between temperature and volume

Question 12: for 1 shot 855 mL of nitrogen gas was collected over water at 781 mmHg and 25oC. The partial pressure of water at 25oC is 23 mmHg. How many moles of nitrogen gas were collected?

Question 12: for 1 shot Nitrogen gas was collected over water at 781 mmHg and 25oC. The partial pressure of water at 25oC is 23 mmHg. How many moles of nitrogen gas were collected?

Question 13: for 1 shot When iron rusts, it undergoes a reaction with oxygen to form iron(III) oxide. 4Fe(s) + 3 O2(g) → 2Fe2O3(s) Calculate the volume of oxygen gas at STP that is required to completely react with 52.0 g of iron.

Question 13: for 1 shot When iron rusts, it undergoes a reaction with oxygen to form iron(III) oxide. 4Fe(s) + 3 O2(g) → 2Fe2O3(s) Calculate the volume of oxygen gas at STP that is required to completely react with 52.0 g of iron.

Question 14: for 1 shot What is the assumption of the kinetic molecular theory that explains why a gas can expand to fill a container?

Question 14: for 1 shot What is the assumption of the kinetic molecular theory that explains why a gas can expand to fill a container? Gases move in constant, rapid, random motion