Answered: A 1.00 L bottle of carbonated soft… | bartleby

Related questions

Question

A 1.00 L bottle of carbonated soft drink contains 5.60 g of carbon dioxide dissolved in it. If the evaporating carbon dioxide is trapped in a cylinder at 1.00 atm and 22.0°C, what volume (in L)
does the gas occupy?
L
Need Help?
Submit Answer
Read It

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Blurred answer

Similar questions

A3] a) Find the temperature of 1 mole of oxygen molecules if they occupy a volume of 4 L and have a pressure of 6 x 10° Pa. You should treat the oxygen as an ideal gas and take the value of the universal gas constant to be R = 8.31J mol1 K-. b) What is the density of the oxygen? You may assume that the mass of I mole of oxygen molecules is 32 g. c) What is the mean square velocity of the oxygen molecules? d) State two assumptions of the kinetic theory of ideal gases that the van der Waals model does not require to be true.
Gas is confined in a tank at a pressure of 9.2 atm and a temperature of 21.5°C. If two-thirds of the gas is withdrawn and the temperature is raised to 85.0°C, what is the pressure of the gas remaining in the tank? ?atm
A hot air balloon holds 7.40 x 107 liters of gas. In order for the hot air balloon to rise into the sky, it must be heated to 120°C. Once the balloon is up in the air, the air needs to be cooled in order for the balloon to land. If the temperature of the balloon is decreased to 40.0°C, what will the new volume of the gas be? SOMEONE PLEASE HELP ME!!
A bicycle tire has a pressure of 6.80 ✕ 105 N/m2 at a temperature of 19.0°C and contains 2.30 L of gas. What will its pressure be (in Pa) if you let out an amount of air that has a volume of 120 cm3 at atmospheric pressure? Assume tire temperature and volume remain constant. _________Pa
The gauge pressure in your car tires is 3.00 ✕ 105 N/m2 at a temperature of 35.0°C when you drive it onto a ship in Los Angeles to be sent to Alaska. What is their gauge pressure (in atm) later, when their temperature has dropped to −42.0°C? Assume the tires have not gained or lost any air. ____atm??
A certain amount of gas at 25.0°C and at a pressure of 0.650 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 2.00 atm. How high can you raise the temperature of the gas without bursting the vessel? In other words, at what temperature will the glass vessel shatter, in degrees Celsius.
A container holds 0.420 m3 of oxygen at an absolute pressure of 3.80 atm. A valve is opened, allowing the gas to drive a piston, increasing the volume of the gas until the pressure drops to 1.40 atm. If the temperature remains constant, what new volume (in m') does the gas occupy? HINT m3 Need Help? Read It Watch It
A hot air balloon uses the principle of buoyancy to create lift. By making the air inside the balloon less dense then the surrounding air, the balloon is able to lift objects many times its own weight. A large hot air balloon has a maximum balloon volume of 2090 m3. a. If the air temperature in the balloon is 54 °C, how much additional mass, in kilograms, can the balloon lift? Assume the molar mass of air is 28.97 g/mol, the air density is 1.20 kg/m3, and the air pressure is 1 atm.
The density of lead is 1.13 x 10“ kg/m³ at 20.0°C. Find its density (in kg/m) at 131°C. (Use a = 29 x 10-° (°C)-- for the coefficient of linear expansion. Give your answer to at least four significant figures.) HINT 3 × kg/m³ 11216.1
#6