1. A rigid-sided flask contains an ideal gas at temperature 460o C and pressure 4.32 atm. If the flask is now heated to 801 oC, find the new pressure inside the flask, in atm.
2. In a certain heat engine: a fuel-air mixture is injected into a cylinder of volume 6.06 cc at pressure 7.08 atm and temperature 383o C. Now a piston comes down, compressing the gas to a volume 3.03 cc and pressure 64.2 atm. Find the Celsius temperature of the fuel-air mixture.
1. A rigid-sided flask contains an ideal gas at temperature 460o C and pressure 4.32 atm....
A flask contains 5 moles of an ideal gas at 25C and 2 atm pressure. The temperature of the gas is raised to 50C. What fraction of the gas must be removed to keep the pressure in the flask constant.
(Gas Pressure; 2pts) A 12-liter flask contains 1.2 moles of an ideal gas at a temperature of 20 degrees Celsius. What is the pressure in the flask in the flask in units of atmospheres? (Round your answer to three significant digits.)
4. A rigid container of 0.2 m3 volume contains a gas at a pressure of 2 bar and a temperature. 25 C. If the characteristic constant for the gas is 0.35 kJ kg-1K-1, calculate: (a) The mass of the gas (b) The pressure of the gas after it is heated to 250°C 4. A rigid container of 0.2 m3 volume contains a gas at a pressure of 2 bar and a temperature. 25 C. If the characteristic constant for the...
5 A rigid tank contains 2 kg of an ideal gas at 4 atm and 40°C. Now a valve is opened and half of mass of the gas is allowed to escape. If the final pressure in the tank is 2.2 atm, determine the final temperature in the tank. Solve this using appropriate software.
Question 3 A rigid tank, of 0.5 m volume, contains an ideal-gas mixture at 300 K. The mixture is made up of 2.4 kg of gas A and 1.4 kg of gas B, the molecular weights of which are MA = 32.0 kg/kmole and M 28.0 kg/kmole, respectively. i. Determine the mass fraction of A and B. (3 marks] ii. Determine the mole fraction of A and B. [5 marks] iii. Determine the molecular weight of the mixture. [2 marks]...
A gas originally at 27 °C and 1.00 atm pressure in a 2.9 L flask is cooled at constant pressure until the temperature is 11 °C. The new volume of the gas is ________ L.
1. What would be the new pressure (in atm.) if a gas sample at 75°C and 2.0 atm. was heated to 100.0°C at constant volume. 2. How many grams of O2 are contained in a 4.0 L sample at 2.0 atm. and 25°C? 3. What is the total pressure of a mixture of N2 and O2 if the partial pressures are 350 mmHg and 475 mmHg, respectively? What is the % of N2 and O2 in the mixture? 4. What...
1- A sample of carbon dioxide gas at a pressure of 1.03 atm and a temperature of 210 °C, occupies a volume of 546 mL. If the gas is cooled at constant pressure until its volume is 443 mL, the temperature of the gas sample will be ______ °C. 2- A sample of nitrogen gas at a pressure of 831 mm Hg and a temperature of 81 °C, occupies a volume of 6.66 liters. If the gas is heated at...
1-If 3.89 moles of an ideal gas has a pressure of 1.42 atm, and a volume of 26.99 L, what is the temperature of the sample in degrees Celsius? 2-A sample of an ideal gas has a volume of 3.40 L at 14.20 °C and 1.30 atm. What is the volume of the gas at 22.40 °C and 0.987 atm? answer____L
The initial temperature of three moles of oxygen gas is 28.0°C, and its pressure is 6.70 atm. (a) What will its final temperature be when heated at constant volume so the pressure is five times its initial value? (b) Now the volume of the gas is also allowed to change. Determine the final temperature if the gas is heated until the pressure and the volume are tripled.