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Consider the following equalibrium: 4NH3(g) + 3O2(g) <--> 2N2(g) + 6H2O(g). Suppose 0.30 mol of NH3 and 0.40 mol of oxygen are added to a 5.0-l container. If x mol of water is present at equalibrium, how many moles of ammonia will remain at equalibrium? Moles of NH3=?
to determine the volume of a gas using ideal gas law.what volume will 5.6 moles of sulfur hexafluoride sf6gas occupy if
A volume of water was delivered using a buret and experimentally determined to have a mass of 2.00-g. What was the final volume of water on the buret if the inital was 0.44-mL? [assume the density of water is 1.00g/mL]
Determine what is Δ[Br- ]/Δt If Δ[BrO 3 - ]/Δt = 0.018 M/s express your answer in M/s?
Solid silicon and solid magnesium chloride form when silicon trichloride gas reacts with magnesium metal. Write a word equation and an unbalanced formula equation.
Calculate the cell potential for the following reaction as written at 53C, given that [Zn2+]= .841M and [Fe2+]= .0160M. Standard reduction potentials are Zn(s)= -.76, Fe2+(aq)= +.771, Zn2+(aq)= -.76, Fe(s)= -.04
The excess I3- was titrated with 50.00 mL of a 0.02000 M Na2S2O3 solution. What was the mass percent of arsenic trichloride in the original sample?
By substituting two hydrogen atoms on the benzene ring with methyl groups, write line-angle formulas of all constitutional isomers. Name each isomer.
Calculate the pH at the equivalence point in the titration of 56 mL of 0.10 M methylamine (see Table 15.4) with a 0.20 M HCl solution.
A 500-g sample of Al2(SO4)3 is reacted with 450 g of Ca(OH)2. A total of 596 g of CaSO4 is produced. What is the limiting reagent in this reaction, and how many moles of excess reagent are unreacted?
What is the minimum uncertainty in the position of an electron, given that we know nothing about its speed except that it is less than the speed of light?
A hydrocarbon undergoes complete combustion to form 6.9 g CO2 and 2.8 g H2O. What is the empirical formula for the hydrocarbon?
Suppose a reaction has a standard Gibbs-free energy of -15.1 kJ/mol, calculate the relative ratio of product to reactant.
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