The mole fraction of oxygen molecules in dry air is 0.186. What volume of dry air at 2.88 atm and 22.1°C is required for burning 2.17 L of octane (C8H18, density = 0.717 g/mL) completely, yielding carbon dioxide and water? Answer=__________

12

8.2 L of chlorine gas at 298 K and 3.0 atm is added to a rigid 4.0 L reaction vessel containing 3.2 moles of He gas and 2.4 moles of fluorine gas?  Chlorine and Fluorine gas react according to the following reaction at 298 K.                                                               Cl2 (g)    +    3 F2  (g)    à 2 ClF3 (g)               What is the partial pressure of ClF3 after the reaction is complete?                If the reaction proceeded with a percent yield of 40%, what would be the partial pressure of ClF3?

A typical sample of air contains 21.0% O2 by volume. For any gas, the volume the gas occupies is directly proportional to the number of moles of gas at a given temperature and pressure. How many moles of oxygen are present in 18.75  moles of air?

Please use SI units and state which corellation is used

How many grams of antifreeze would have to be added to 15 kg of water in the trucks cooling system to keep it from freezing during a cold Ohio winter temperatures of -20° C

Example 3: A vessel content, one mole of carbon dioxide is heated. The carbon dioxide is dissociated 1 as: CO₂ → CO + 0₂. 2 If the equilibrium constant is given as: Kp = 30 ln(T) – 240. After equilibrium occurs, the carbon monoxide mole fraction is 0.098 find the reached temperature of the mixture.

P2

Use the information about three gases, with the properties below to answer the following questions. Nitrogen (N2) Oxygen (02) Argon (Ar) 93.0 °C 83.0 °C 73.0 °C M (kg/kmol) 28 32 40 Use the van der Waals equation of state and mixing rules to calculate the temperature where 100 kmol of a mixture of argon (10 mol%), nitrogen (45 mol%) and oxygen (45 mol %) would occupy 46.27 m³, at a pressure of 6.28 MPa. It is known that the van der Waals constant for nitrogen are a=1.370 atm(m³/kmol)² and b=0.0387 m³/kmol, and for oxygen are a=1.382 atm(m³/kmol)² and b=0.03186 m³/kmol. 63.0 °C Tc (K) 126.2 154.6 150.8 Pc (atm) 33.5 49.8 48 @ 0.04 0.021 -0.004

Calculate the vapor phase mole fractions in equilibrium with a liquid hydrocarbon binary mix of 42% carbon tetrachloride and 58% trichloroethylene (use Antoine equation to calculate vapor pressures), for a system at 60°  Also, calculate what is the total system pressure?