In a 2.29 L flask, there are two gases (gas 1 and gas 2). There is 2.13 L of gas 1, with 3.7 bars of pressure, and there is 6.04 L of gas 2, with 8.16 bars of pressure. In the flask mixture, find the final pressure value in bars, and assume that temperature is held the same for both gases and that both gases behave ideally.

Please pick one of the multiple choice answers.

7. Suppose we have a 12.2 L sample containing 0.50 mol of oxygen gas (O2) at a pressure of 1 atm and a temperature of 25oC. If all of this is converted to ozone (O3) at the same temperature and pressure, what will be the volume of the ozone?

At 58 C, the volume of a gas is 53.2 mL.  At the same pressure, its volume is 154 mL at what temperature?

1. A. If all of the nitrogen gas produced from the rocket fuel in problem 1 is placed in a 50.00-L tank at 74.1 °C, what will the pressure inside that flask be in atmospheres? B. A common rocket propellant is a mixture of dinitrogen tetroxide and unsymmetrical dimethylhydrazine. When combined, they react violently to produce several gases and a great deal of heat, as shown. If 500. g of C2H8N2 and 600. g of N2O4 react, how many grams of nitrogen gas will be produced? Which is the limiting reactant? C2H8N2(l) + 2 N2O4(l) ——> 3 N2(g) + 2 CO2(g) + 4 H2O(g)

A 13.0 L sample of hydrogen gas has a pressure of 21.0 atm at a certain temperature. At the same temperature, what volume would this gas occupy at a pressure of 4.10 atm? Assume ideal behavior. ?=                 L

2. A sample of helium occupies a volume of 2.5L at a pressure of 525 kPa. If the temperature of the gas is kept constant, what would the new volume of the gas be at 415 kPa?

A mixture of nitrogen and carbon dioxide gases, in a 6.15 L flask at 59 °C, contains 2.64 grams of nitrogen and 11.7 grams of carbon dioxide. The partial pressure of carbon dioxide in the flask is  atm and the total pressure in the flask is  atm.

A 2.20 L container at 53.6 °C contains 6.21g N2⁢O3⁡(g). The N2⁢O3 gas decomposes completely, producing NO2⁢(g) and NO(g). Assuming the container volume and the temperature do not change, calculate the pressure of the gas mixture after the complete decomposition of N2O3.

A sample of xenon gas occupies 71.1 litres under a pressure of 1.55 x 103 torr at 25.0 °C. What volume (in litres) would this sample occupy at -72.8 °C, if the pressure remained constant? Assume xenon acts as an ideal gas. Enter the numerical value (no units), using 3 significant figures. Type your answer...