Popcorn pops because the kernel contains water that turns to steam when the kernel is dropped into hot oil; when the steam expands it pops the kernel. Given that the mass of a popcorn kernel is 0.125 g and that the water is 13.5% of the mass of the kernel. Assume that all the water turns to steam, and use that mass for further calculations. If the temperature is 240 oC when the kernel is popped, calculate the pressure in kPa that is generated by the water when it turns to steam and pops the kernel. Show

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 .

9.26 mol of argon gas is admitted to an evacuated 4,546.84 cm3 container at 38.34oC. The gas then undergoes an isochoric heating to a temperature of 293.66oC. What is the final pressure?

A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. The vessel is a stainless-steel cylinder that measures 21.0 cm wide and 25.2 cm high. The maximum safe pressure inside the vessel has been measured to be 8.80 MPa. For a certain reaction the vessel may contain up to 0.650 kg of carbon dioxide gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. Write your answer in degrees Celsius. Round your answer to 3 significant digits. temperature: I °C

A gas sample has a mass of 1.211 g and occupies a volume of 677 mL. The temperature in the laboratory is 23 ⁰C and the gas pressure is 100. kPa. What is the molar mass of the gas?

In an air-conditioned room at 21.0 ∘C, a spherical bubble had the diameter of 60.0 cm. When taken outside on a hot summer day, the bubble expanded to 61.0 cm in diameter. What was the temperature outside in degrees Celsius? Assume that the bubble is a perfect sphere and that the pressure and number of moles of air molecules remains the same.

Calculate the temperature in oC for a 1.9 moles of carbon dioxide in a 1,290 mL container at a pressure of 495.2 kPa. Note: R = 0.08206 L atm/(K mol).

When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete - the lime absorbs CO₂ from the air and turns back into hard, durable limestone. Suppose a limekiln of volume 800. L is pressurized with carbon dioxide gas to 14.9 atm, and heated to 960.0 °C. When the amount of CO, has stopped changing, it is found that 3.96 kg of CaCO, have appeared. Calculate the pressure equilibrium constant K, this experiment suggests for the equilibrium between CaCO3 and CaO at 960.0 °C. Round your answer to 2 significant digits. Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for K, does not match the accepted value. K = 3.07 P