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At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must be added at constant temperature and pressure if you need a total of 1.00 mol of oxygen gas in the vessel?
The orbital energy of any atomic species depends on factors other than the principle quantum number n and any given energy level in H is more stable than the same level in H+.
How much heat (in kJ ) is required to warm 12.0 grams of ice, initially at -12.0 Celsius, to steam at 112.0 Celsius? The heat capacity of ice is 2.09 J/g*Celsius and that of steam is 2.01 J/g*Celsius?
A 2L cylinder of gas contains 2.4 moles of gas at 34 degrees Celsius. What is the pressure?
The gas phase irreversible first-order reaction A----> 3B , is carried out in PFR where the feed is equal molar in A and inerts. the conversion under these circumstances is 50%.
Constant external pressure of3.00 atm, followed by2) against a constant external pressure of 2.00 atm. Calculate q and w. (101.33 J = 1 L atm)
The stopcock between a 3.00 L bulb containing oxygen at 295 torr and 1.00 L bulb containing nitrogen at 530 torr is opened. What is the total pressure of the mixture.
How many liters of 13.5 molar HCl stock solution are needed to make 10.5 liters of a 1.8 molar HCl solution?
The rate of disappearance of HBr in the gas phase reaction is 0.103 Ms-1 at 150 deg Celsius. what is the rate of reaction.
the enthalpy of vaporization of ethanol i 43.5 kj/mole at its normal boiling point of 352 k. using avalue of the molar heat capacity of liquid ethanol of 111.46 j/k/mol
A cylinder of oxygen gas contains 26.4 g of O2. Another cylinder, twice the volume of the cylinder containing oxygen (and at the same conditions of pressure and temperature), contains CO2 gas.
Determine what would be the total ?nal pressure of the system in atmospheres If we completely hydrolyzed 0.18 kg of H2O in a 8.2 L container at 300 K?
15.0 moles of gas are in a 5.00L tank at 22.2°C. compute the difference in pressure between CH4 and an ideal gas under these circumstances. The van der Waals constants for CH4 are a=2.300L2⋅atm/mol2 and b=0.0430 L/mol.
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