A can of hair spray is used until it is empty except for the propellant, isobutane gas.(a) On the can is the warning “Store only at temperatures below 120 °F (48.8 °C). Do not incinerate.” Why?(b) The gas in the can is initially at 24 °C and 360 kPa, and the can has a volume of 350 mL. If the can isleft in a car that reaches 50 °C on a hot day, what is the new pressure in the can?

A 9.00 L tank at 12.6 °C is filled with 7.50 g of carbon dioxide gas and 13.2 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: x10 carbon dioxide partial pressure: || atm ? mole fraction: dinitrogen difluoride partial pressure: atm Total pressure in tank: || atm

I need help with the problem set.

In order to produce solid iron, it first must bc processed from its orc, Fe2O1, in a blast furnace. During operation, CO gas (flue gas) is introduced into the furnace at 1650 °C and a pressure of 250 kPa. In this process flue gas reduces iron to its elemental form in the following reaction: 41. Fe;O30) COg Fe+ COz At one point in this process 256.0 L of CO was used to reduce iron ore. Assuming a complete reaction, how many grams of solid iron can be produced. Balanced chemical equation: Mass of Fe (in grams)

5. There are 1.07 X 103 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)

There are 1.07 X 10-3 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure.  After several uses, the internal pressure is 3.4-atm.  How many moles of gas remain in the cartridge?  How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)

If 6 g of ethane is burned in oxygen, then How many moles of water and carbon dioxide are formed? If the aforementioned products reaction is diverted in one tank, where the temperature of the tank is above 100°C, then what is the volume of tank required to store the gases? If the temperature is below 100ºC, then how much volume of gas will form? (Assume the pressure of tank = 2atm, and temperature of tank in (b) is 120°C and in (c) is 25°C)

A 100-liter empty jar was spiked with 20 mg of TCE (C2HCl3) under room temperature condition. The jar was then closed tightly. What is the concentration (in atm.) of TCE in the air at 25 C? (TCE: MW: 131.4 g/mol; TCE solubility in water (Cs) = 1100 mg/L; Pv (pure liquid at 25oC) = 10^-1.01 atm. KH = 10^1.03 L atm mol-1; KOW = 102.42).  if the jar was half filled with water and half filled with air, what were the concentrations of TCE in both air and water at 25C?

Hot gaes Expanding A mixture hot gases expands, changing volume from 2.45 L to 6.82 L, against a constant pressure of 3.22 atm. The P-Vwork involved is Latm .

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.