A spray can is used until it is empty except for the propellant gas, which has a pressure of 1344 torr at 23 °C. If the can is thrown into a fire (T = 475 °C), what will be the pressure in the hot can?

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)

The average kinetic energy of the molecules in a gas sample depends only on the temperature, T. However, given the same kinetic energies, a lighter molecule will move faster than a heavier molecule, as shown in the equation for rms speed 3 RT rms speed where R = 8.314 J/ (mol·K) and M is molar mass in kilograms per mole. Note that a joule is the same as a kilogram-meter squared per second squared (kg-mIs²). What is the rms speed of O, molecules at 307 K? rms speed: m/s What is the rms speed of He atoms at 307 K? rms speed: m/s

Using the ideal gas law (PV=nRT), calculate the temperature of a gas in a canister 10.4 L in volume. The pressure is 234,567 Pa and there are 32 moles.  (R= 0.0821 L atm/ mol K) (101,325 Pa/1 atm).

How many moles of gas must be forced into a 3.1 LL ball to give it a gauge pressure of 8.4 psipsi at 23 ∘C∘C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.6 psipsi so that the total pressure in the ball is 23.0 psipsi .

For the following reaction: C3H8(g) + 3CO₂(g) + 4H₂O(1) 502(g) The change in gaseous moles, An = To maximize the product yield, the volume of the container should ◆ , so that the pressure will be (> →

Consider the following situation:  You have a 50 L tank of compressed air at 15 atm and 100 ºC.  You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal.  The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania).  Once the purified air is passed through the getter is it cooled back down to  100 ºC and fills another 50 L storage tank.  If air typically contains about 20% oxygen, what could the pressure in the storage tank be?     Question 2 options:   A)  12 atm   B)  15 atm   C)  18 atm   D)  24 atm

5. Does the pressure-volume relationship follow the ideal gas law PV=nRT (is PV constant at constant n and T) Using the room temperature calculate the number of moles in the pressure/volume experiment when the pressure is 1.00atm in 3.1

Consider the reaction shown below: 2 HCl (aq) + CaCO3 (s) ⟶ CO2 (g) +  CaCl2 (aq) + H2O (l) How many grams of CaCO3 would need to be consumed to fill a 908.001 mL balloon with CO2 gas, assuming a constant temperature of 21.7 oC and constant pressure of 0.958 atm? Express your answer in units of grams using at least three significant figures.