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if you had excess chlorine how many moles of of aluminum chloride could be produced from 17 grams of aluminum
How many grams of F2 are needed to produce 120. g of PF3 if the reaction has a 78.1% yield?
Calculate delta E for the combustion of a gas that releases 195.0 kJ of energy to its surroundings and does 54.5 kJ of work on its surroundings.
If 23mL of 6.4M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid.
Calculate the enthalpy change for the dissolution of NH 4 NO 3 and expree your answer in units of kJ/mol.
What is the pH of the solution if [OH-] of an ammonia solution is 1.0 X 10-2M?
What mass of HCl is contained in 30.0ml of a solution solution which is 37.2 mass% HCl has a density of 1.19g/ml.
A sample of nitrogen (9.27g) reacts completely with magnesium, according to the equation: 3 Mg + N2 -> Mg3N2. The mass of Mg consumed is ____g?
Calculate the equilibrium constant (Keq) for the reaction of equimolar amounts of acetophenone and sodium hydroxide to generate the enolate.
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s). If 12.5 g of iron(III) oxide (rust) are produced from 8.74 g of iron, how much oxygen gas is needed for this reaction?
Dry ice (solid CO2 ) has occasionally been used as an "explosive" in mining. A hole is drilled, dry ice and a small amount of gunpowder are placed in the hole, a fuse is added, and the hole is plugged.
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
If this energy were used to vaporize water at 100.0 degrees, how much water (in liters) could be vaporized.
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