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Given the reaction 4Al(s)+302(g)--2Al2O3(S), what is the minimum number of moles of oxygen gas required to produce 1.00 mol of aluminum oxide?
How much energy is released from the complete combustion of 63.0 g of sulfur in this equation:
a 100 g sample of water at 23C is added to a 45 g sample of water at 99C. what is the final temperature of the sample
A gas held at 798 mmHg in a 400 mL flask is released into a 3 L flask.Whats the new gas pressure?
Calculate the number of carbon atoms in 0.75 L of acetone (CH3COCH3). (density = 1.3 g/mL and boiling point = 48.5 degrees Celsius)
What volume will contain 5.0 mol of aluminium? The density of aluminium is 2.7 g/ml.
Write the formula of the reactants and products-including the symbols for the state- (s), (l), (g), (aq)- then balance the equation.
Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21
At some temperature, a chemist found the following equilibrium concentrations. [Fe3+] = 6.63 10-3 M, [SCN-] = 7.36 10-3 M, [FeSCN2+] = 4.34 10-2 M
Assume that the heat was completely absorbed by the water and no heat was absorbed by the reaction container or the calorimeter or lost to the surroundings. Calculate the Hrxn per mole of SiH4.
The heat of vaporization of benzene, C6H6 , is 30.8 kJ/mol at its boiling point of 80.1 °C. How much heat is required to vaporize 128 g benzene at its boiling point ?
The enthalpy of combustion of methane, Ch4, is -890 KJ/mol. If the gas flow rate of the methane to the burner of a stove is 5 L/min at 25 degrees celsius and assuming complete heat transfer from combustion
If 164 of wet is collected over water at 24 degrees C and a barometric pressure of 737 Torr , how many grams of Zn have been consumed? (The vapor pressure of water is 22.38 Torr)
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