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A mercury mirror forms inside a test tube by the thermal decomposition of mercury(II) oxide. 2 HgO(s) 2 Hg(l) + O2(g) Hrxn = 181.6 kJ (a) How much heat is needed to decompose 504 g of the oxide? kJ? (b) If 282 kJ of heat is absorbed, how many grams of mercury form? g?
Determine the heat of combustion per gram of octane and the heat of combustion per mole of octane?
H2SO4, for the first step instead of concentrated HNO3 . What changes will be observed for the initial reaction with copper metal?
When a magnetic sector instrument was operated with an accelerating voltage of 2500 V, a magnetic field of 0.4 Tesla was required to focus on the CH4+ on the detector.
Calculate q if the temperature of a 1.00 kg water bath in the surroundings increases by 1.25 Celsius degree.
Calculate the mass of the reaction mixture in the calorimeter. (To do this, assume that the density of the HCl solution originally in the calorimeter can be approximated with the density of water (1.0 g/mL).
Why might this fire rekindle days later as someone tries to remove the residue with water? What chemical process is involved here?
Hydrochloric acid is added to zinc. How many mls of 0.500 M HCl are needed to react completely with 25.0 g of zinc metal
How many grams of N2 are required to react with 2.30 moles of Mg in the following process?
Careful spectral analysis shows that the yellow light of the sodium lamp is made up of photons of two wavelengths, 589.0 nm and 589.6 nm. What is the difference in energy (in joules) between photons with these wavelengths?
The products of a specific reaction and the side products or impurities? Explain specifically what would be observed for this pair of compounds: 4-bromoacetanilide and 2-bromoacetanilide
Determine How hot should be the air in a ballon be heated if it has initially a volume of 750. L at the temperature of 20 degree celsius and the final volume must be 1,000.l
Determine the oxidation number for the indicated element in each of the following substances.
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