A container with a volume of 1.60 L was evacuated and then filled at low temperature with 0.0460 mol liquid dinitrogen tetroxide N2O4,. As the temperature was raised, this substance formed nitrogen dioxide N02,: If the pressure of this reaction mixture at equilibrium at 25.0°C was 0.848 atm, what was the total moles of gas in this mixture? 0.0554 MOL What are the moleS of NO2 and moles of N2O4? 0.0188 mol of NO2 0.0366 mol of N2O4     What are the partial pressures of NO2  and N2O4?   Partial pressure of NO2=______atm? Partial pressure of N2O4=_______atm?

The following reaction is investigated (assume an ideal gas mixture): 2N20(g) + N2H4(g) 3N2(g) + 2H2O(g) Initially there are 0.100 mol of N20 and 0.25 mol of N2H4, in a 10.0-L container. If there are 0.059 mol of N20 at equilibrium, how many moles of N2 are present at equilibrium? O 4.1 x 10^-2 1.2 x 10^-1 6.2 x 10A-2 O 2.1 x 10^-2 O none of these

Use the following equilibrium. H2(g) + CO2(g)  H2O(g) + CO(g)    K = 16.0 The initial partial pressures of H2 and CO2 in the reaction flask are each 1.80 atm. What is the equilibrium pressure of CO?  atmWhat is the final total pressure at equilibrium?  atm

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 2.0 L flask with 3.1 atm of carbon monoxide gas and 3.6 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 1.0 atm of carbon monoxide gas, 1.5 atm of water vapor and 2.1 atm of carbon dioxide. The engineer then adds another 0.90 atm of water, and allows the mixture to come to equilibrium again. Calculate the pressure of hydrogen after equilibrium is reached the second time. Round your answer to 2 significant digits. 0 atm x10 C [