When gaseous F₂ and solid I₂ are heated to high temperatures, the I₂ sublimes and gaseous iodine heptafluoride forms. 3.20 × 10² torr of F₂ and 2.90 g of solid I₂ are put into a 2.50 L container at 2.50 × 10² K and the container is heated to 5.50 × 10² K. (a) What is the final pressure? Ptotal (b) What is the partial pressure of I₂ gas? P1₂ atm atm 1₂

8) Consider the apparatus pictured below, which consists of two containers separated by a valve. CH;N(g) 285 mL O2(g) 419 mL 591 torr 1766 torr The valve is opened and the gases react as follows (note that the temperature is high enough that the water is produced as a gas): 4 C2H;N(g) + 15 O2(g) → 8 CO2(g) + 14 H2O(g) + 2 N2(g) What will be the total pressure in the apparatus when the reaction has gone to completion? Assume that the temperature does not change.

A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)

A gaseous “CFC” compound has a density of 5.456 g/L at 0.993 atmand 22.0oC. (a) Calculate the molar mass of the compound. (b) If the compound has the following composition: 18.10% C; 28.60% F, and 53.30% Cl, by mass, determine the molecular formula of the compound. (CFC = chlorofluorocarbon)

4.)  (a)  0.375 g of CO2 gas is held in a 520.-mL container at 24. oC.  What is its pressurre?                                                                                                                                    atm (b) 0.375 g of N2 are held in an identical container at the same temperature.  What is its pressure?                                                                                                                           atm (c) Are the pressures the same or different?  Why?                                                                                         (d) If both these samples were contained in the same 520.-mL container, what would the partial pressure of each gas be?  What would the total pressure be? (FYI, these gases do not react.)       PCO2=                          atm                                                                                                                                     PN2=                            atm…

0.300 mol of O2 gas is held at an a 5.00 L container at 45.0 °C. Determine the following:(a) the volume this gas occupies at ST (in L).(b) the pressure of this gas if the temperature isincreased to 60.0 °C assuming the volume does notchange.(c) the volume of NO2 (in L) expected from complete combustion of the excess N2 in O at STP.Hint: Use answer from (a) as a starting point.

The flame produced by the burner of a gas (propane) grill is a pale blue color when enough air mixes with the propane (C3H8) to burn it completely. For every gram of propane that flows through the burner, what volume of air is needed to burn it completely? Assume that the temperature of the burner is 205.0°C, the pressure is 1.05 atm, and the mole fraction of O2 in air is 0.210.

11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b)  The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.

7a