1.0 mole of N2, 0.75 mol O2, and 0.50 mol H2, each at 25°C and 2 bar, are mixed isothermally. The final pressure is 2 bar. Calculate ∆S and ∆Ssurr, on the assumption of ideal behavior.
11. A 25 L flask at 25°C contains 0.75 mol of N2, 0.50 mol of O2 and 1.25 mol of CO. What is the total pressure? e) 500 atm a) 0.0082 atm b) 2.4 atm c) 21 atm d) 250 atm
A vessel of volume 22.4 dm3 contains 2.0 mol H2(g) and 1.0 mol N2(g) at 273.15 K. (a) Calculate the mole fractions of each component. H2 N2 (b) Calculate the partial pressures of each component. H2 N2 (c) Calculate the total pressure.
A 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0˚C. a. What is the total pressure in the flask? b. What fraction of the total pressure in the flask is due to N2? c. If the temperature of the flask is lowered, what happens to the pressure inside the flask? d. On a molecular level, explain why the pressure changes as you predicted in part (c). e. If...
A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.
calculate U and H when the pressure of 0.02 mol of an ideal gas at 2 bar and 0.25 L is reduced to 1 bar and 0.25 L. calculateU andH when the volume of 0.02 mol of an ideal gas at 1 bar and 0.25 L is increased to 1 bar and 0.50 L. calculateU andH when 0.02 mol of an ideal gas at 2 bar and 0.25 L is expanded to 1.0 bar and 0.50 L isothermally.
7-A gas mixture consists of N2, O2, and Ne, where the mole fraction of N2 is 0.50 and the mole fraction of Ne is 0.20 If the mixture is at STP in a 3.0 L container, how many molecules of O2 are present? 8-Calculate the density of Freon-12, CF2Cl2, at 37.0°C and 0.369 atm. 9-Determine the final temperature of a gold nugget (mass= 256 g) that starts at 378 K and loses 5.37 kJ of heat to snowbank when it...
2. The pressure dependence of the following system at equilibrium was studied at 500°C by measuring the mole fractions of ammonia that were produced at various pressures from 1:3 mixtures of N2 and H2 gases. Assume ideal gas behavior. (Hint: You may assume that the mixtures were prepared from 1 mole of N2 mixed with 3 moles of H2). (10 pts) Ng(g)+H,(g)P NH,(g) P/(bar) 100 XNH3 0.10 200 0.18 300 0.25 400 0.32 500 0.37 600 0.42 700 0.46 800...
7.0 L of O2 at 1.0 atm is mixed together with 8.0 L of N2 at 7.0 atm at a constant temperature of 25 C in a 25.0 L vessel. What is the mole fraction of N2 in the 25.0 L vessel? Assume the gases behave ideally. Express your answer as a unitless mole fraction using at least three significant figures.
A quantity of 0.50 mole of an ideal gas at 20°C expands isothermally against a constant pressure of 2.0 atm from 1.0 L to 5.0 L. Calculate Asus ASgurr and AS (1 L.atm = 10133 J) Select one or more: A. 12.7 J/K, -9.7J/K 3.0 JAK B.22.4 J/K -34.3 J/K -11.9 J/K C. 6.7 J/K -2.8 J/K 3.9 J/K D. -6.7 J/K, 6.7 J/K 0.0 JIKE An adult human brain operates at 25 Watt (1 Watt - 1 J/s) for...
Question 2 One mole of an ideal gas, initially at 30 C and 1 bar is changed to 130 °C and 10 bar by using two different mechanically reversible processes: 2.1 The gas is first heated at constant pressure until its temperature is 130 °C and then compressed isothermally to 10 bar. 2.2 The gas is first compressed isothermally to 10 bar and then heated at constant pressure to 13°C Calculate Q, W, AU, and AH for each case. Take...