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Assuming that the total pressure of the gases is 1.52 and that their mole ratio is 94 : 4.0 : 1.5 : 0.50, calculate the partial pressure (in atmospheres) of each gas.
A balloon has a volume of 10,500 liters, and the temperature is 15°C. If the temperature were -25°C, what would the volume of the balloon be?
The reported values for one compound (CaHbOc) were as follows: mass: 214.1360 g/mol; percent C and H: 84.07 and 8.47, respectively. Determine the molecular formula of the compound.
How many grams of water should be produced and What is the theoretical yield of nitrogen?
Determine the mass of precipitate (in grams) that forms when 213.8 mL of 0.132 M CaCl2 solution is reacted with excess AgNO3 solution.
a metal weighing 50.0g absorbs 220.0 J of heat when its temperature increases by 120.0 degrees celsius. what is the specific heat of this metal?
Calculate the pH for each of the following cases in the titration of .50 mL of .150 M hypochlorous acid, HCLO(aq)
Using a solution of (HOC 2 H 2 )3NHCl, solution in which Kb, ((HOC 2 H 2 )3N) = 5.9 × 10 -7 then determine what is the pH of a 0.010 M triethanolammonium chloride,
Calculate the mass fractions of the components in the mixture and the average molecular weight of the gas mix. b)The gases are mixed with 20% excess air and completely combusted with 100% conversion
Mg3N2(s) + H2O(l) → Mg(OH)2(s) + NH3(g) If this process is 82% efficient, what mass of ammonia can be prepared from 22.0 kg magnesium nitride.
Calculate concentration of NaClO solution from that equation and calculate How many grams of this nuclide in a sample of 4.00 g will remain after 112 years?
How many grams of are CaH2 needed to generate 147L of H2 gas if the pressure of H2 is 827 torr at 20 C?
Write the balanced net ionic equations for the reactions that occur in each of the given cases as. Cr2(SO4)3(aq) + 3(NH4)2CO3 (aq) = Cr2(CO3)3 ( s) + 3(NH4)2SO4 ( aq).
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