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...
molar 7. How many grams of CO 28.01 /mol) must be bumed to produce 225 kJ of heat urma 2006 +020 200260 AH = -566 kJ c) 2238 ite a) 0.398 8 b) 0.795 g c) 2.52 g d) 11.1 g 3. Calculate the mass of excess reactant remaining after 4.50 mol of LHCO (67.96 R/mol) and 8.50 mol of H2504 (98.08 g/mol) reacted according to the equation shown below. 2LHCO3 + H2SO4 - Li2SO4 + 2H20 + 2002 e)...
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.
At 0 ⁰C, each cubic centimeter of a 1.0-L flask contains 5.0 × 10-2 mol of N2, 1.5 × 102 mg O2, and 5.0 × 1018 molecules of NO. What is the partial pressure of each gas, and what is the total pressure in the flask? a. 3400000 atm (total pressure) b. 1.2 atm c. 110 atm d. 1.4 atm e. 1.1 atm f. 3400000 atm g. 0.11 atm h. 1100 atm i. 1200 atm j. 0.19 atm
What is the total pressure in a 9.00-L flask which contains 0.127 mol of H2(g) and 0.288 mol of N2(g) at 20.0°C?a) 0.340 atmB) 0.769 atmC) 0.681 atmD)1.11 atm
please help due tonight 3. A flask contains 0.10 mol of O2 and 0.30 mol of Nz. The total pressure of gas inside the container is 2.4 atm. Calculate the mole fraction of O, and the partial pressure of Oz inside the container
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 22.4 L container at 0 °C contains 0.27 mol N2, 0.19 mol O2, 0.42 mol He, and 0.050 mol CO2. What are the partial pressures of each of the gases in atm, torr, and bar