A closed bottle has a volume of 2 L (1 L air and 1 L water). The air is a mixture of N2 (75%), O2 (20%) and CO2 (5%). The pressure of the air is 1 atm. Determine the pH of the water at equilibrium.
Suppose that Daniel has a 2.50 L bottle that contains a mixture of O2, N2, and CO2 under a total pressure of 5.40 atm. He knows that the mixture contains 0.290 mol N2 and that the partial pressure of CO2 is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O2? PO2= atm
Suppose that Daniel has a 3.00 L bottle that contains a mixture of O2 , N2 , and CO2 under a total pressure of 5.30 atm. He knows that the mixture contains 0.310 mol N2 and that the partial pressure of CO2 is 0.350 atm. If the temperature is 273 K, what is the partial pressure of O2 ?
Suppose that Daniel has a 2.50 L bottle that contains a mixture of O2, N2, and CO2 under a total pressure of 4.70 atm. He knows that the mixture contains 0.23 mol N2 and that the partial pressure of CO2 is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O2?
A student has a 2.68 L bottle that contains a mixture of O2 , N2 , and CO2 with a total pressure of 4.73 bar at 298 K . She knows that the mixture contains 0.273 mol N2 and that the partial pressure of CO2 is 0.306 bar . Calculate the partial pressure of O2 .
0.75 L bottle is cleaned, dried, and closed in a room where the air is 24°C and 38% relative humidity (that is, the water vapor in the air is 0.38 of the equilibrium vapor pressure at 24°C). The bottle is brought outside and stored at 0.0°C. (a) What mass of water condenses inside the bottle? (b) Would water condense at 10°C?
The Haber process { 2 N2(g) + 3 H2(g) <-> 2 NH3(g) } has a Kp of 4.34 x 10^−3 at 300 K. Calculate the pressure of ammonia that is present at equilibrium if we start with 10 atm of nitrogen and 20 atm of hydrogen gas. Predict whether this concentration would increase or decrease if the original mixture was contained in a 5 L metal bottle and the mixture was allowed to expand into a second 5 L bottle,...
Air is a mixture of gases with the following mass percentage composition: 75.52% N2, 23.15% O2, 1.28% Ar, and 0.046% CO2 (a) What are the partial pressures of N2, O2, Ar, and CO2, when the total pressure is 1.100 atm? (b) Calculate the molar Gibbs energy of mixing of air at 25 °C assuming ideal-gas behavior. (c) Determine the molar enthalpy of mixing and the molar entropy of mixing for air at 1.100 atm and 25 °C. 5. (3 pts)...
A vessel initially containing 1 kmol of CO and 4.76 kmol of dry air forms an equilibrium mixture of CO2, CO, O2, and N2 at 2800 K, 1 atm. Determine the equilibrium composition.
***Please type answer if possible*** GAS VOLUME STOICHIOMETRY PROBLEMS 1. The combustion of ethanol (C2H5OH) takes place by the following reaction equation. C2H5OH (l) + 3 O2 (g) → 2 CO2 (g) + 3 H2O (g) What is the volume of CO2 gas produced by the combustion of excess ethanol by 23.3 grams of O2gas at 25oC and 1.25 atm? GAS VOLUME STOICHIOMETRY PROBLEMS 2. Acetic acid (CH3COOH) is formed from its elements by the following reaction equation: ...