For a rigid diatomic molecule, universal gas constant R = nCp where 'Cp' is the molar specific heat át constant pressure and 'n' is a number. Hence (n) is equal to A) 0.2257 C) 0.2857 B) 0.4 D) 0.3557
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- Assume you are using the attached pressure gauge and a thermocouple with a temperature uncertainty of +/- 1C; assuming ideal gas how accurately can you report the molar volume n/V=RT/P?A sealed 19 m3 tank is filled with 7,011 moles of ideal oxygen gas (diatomic) at an initial temperature of 292 K The gas is heated to a final temperature of 490 K. The atomic mass of oxygen is 16.0 g/mol. The final pressure of the gas, in MPa, is closest to: answer round to 4 sig.figPlease asap
- A gas originally occupies a volume of 0.5m^3 at a pressure of kPa. It is slowly allowed to expand until the volume is 2.5m^3. Assuming the temperature is kept constant, calculate the final pressure of the gas.Problem 3. The viral coefficients of a gas at 20 °C and 11.5 bar are B = -138 cm³ mol¹ and C=7222 cmº mol². Calculate the V (molar volume) Z (compressibility factor) of the gas. Use the equation below (R = 83.14 cm³ bar mol-¹ K-¹). PV 2 = ² = (1 + = + =) Z RTA 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.