Question 20 A volume of gas starts at a pressure of 10 atmospheres (atm) and a temperature of 27°C. If the temperature is increased by 75°C and the volume of the gas remains constant, what is the new pressure? 0000 12.5 atm 7.5 atm 27.8 atm 37.8 atm

Four closed tanks, A, B, C, and D, each contain an ideal gas. The table gives the absolute pressure and volume of the gas in each tank. In each case, there is 0.19 mol of gas. Using this number and the data in the table, compute the temperature of the gas in each tank. Absolute pressure (Pa) Volume (m³) A 25.0 4.0 B 30.0 5.0 C 20.0 5.0 D 2.0 75

I need help with this question

0.52 mol of argon gas is admitted to an evacuated 3.00 liter (3.00 × 10-3 m3) container at 20.0°C. The gas then undergoes an isobaric process to a temperature of 260°C. What is the final volume of the gas, in liters? Your answer needs to have 3 significant figures, including the negative sign in your answer if needed. Do not include the positive sign if the answer is positive. No unit is needed in your answer, it is already given in the question statement.

The volume of a gas at 20°C is 100cm3 at normal pressure. If it is heated to 100°C, its volume becomes 125cm3 at the same pressure, then volume coefficients of the gas (at normal pressure) is? a) 0.0033/°C b) 0.0025/°C c) 0.0030/°C d) 0.0021/°C

15.01 A cylindrical tank has a tight-fitting piston that allows the volume of the tank to be changed. The tank originally contains 0.100 m3m3 of air at a pressure of 3.10 atm. The piston is slowly pulled out until the volume of the gas is increased to 0.390 m3 . If the temperature remains constant, what is the final value of the pressure? Express your answer in atmospheres.

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

n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.135 m3   Part (a)  The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas?        Part (b)  The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas

A rigid tank contains an amount of argon at a pressure of 12.2 atm and a temperature of 23.0°C. Two-thirds of the gas is withdrawn from the tank, while the temperature of the remainder is raised to 36.8°C. What is the new pressure (in atm) of the gas remaining in the tank? atm