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How many moles of N2 are produced by the decomposition of 1.40 of NaN3 ?
Suppose 5.00g of Ca is added to 50.0mL of 1.00M HCL. Determine the limiting reactant in this case and number of moles of calcium actually consumed.
How many kilograms of sodium fluoride would be needed to treat an 8.25x10^7 gal reservior?
Write balanced chemical equations for the following reactions.
If the mass of the ore from which the gold was extracted is 166.0 g, what percentage of the ore is gold.
Calculate the ratio of rates of effusion of O2 versus Cl2. Record your answers to three significant figures. The concentration of CO2 in the atmosphere is 375ppm (by volume). What is the mole fraction of CO2 in the atmosphere?
What liquid is insoluble in water and soluble in cyclohexane and alcohol; and has a boiling pint of 58 degress Celsius at 670 mm Hg.
Determine the minimum mass of Sodium bicarbonate or sodium hydrogen carbonate that should be added to the spill to neutralize it?
Calcium hydride, CaH2, reacts with water to form hydrogen gas. CaH2(s) + 2 H2O(l) → Ca(OH)2(aq) + 2 H2(g)
What is the molecularity of the following elementary reaction? NH2Cl(aq) + OH¯(aq) -> NHCl¯(aq) + H2O(l)
Hydrogen and iodine gases react to form hydrogen iodide gas. H2(g) + I2(g) → 2 HI(g) At a certain temperature and pressure 0.70 L of H2 reacts with 0.70 L of I2.
Calculate the enthalpy change in kJ when 19.1g of H2S is burned. 2H2S(g) + 3O2(g) --> 2SO2(g) + 2H20(g) Change in H= -1036kJ/mol
An iron bar of mass 869 - g cools from 90 oC to 5 oC Calculate the heat released (in kilojoules) by the metal. ( specific heat = 0.44 J/(g. c)
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