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Chapter 3: Problem 85

There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating \(0.6498 \mathrm{~g}\) of one of the compounds leaves a residue of \(0.6018 \mathrm{~g}\). Heating \(0.4172 \mathrm{~g}\) of the other compound results in a mass loss of \(0.016 \mathrm{~g}\). Determine the empirical formula of each compound.

Short Answer

Expert verified
The empirical formula of the first compound is \(Hg_1O_2\) (mercury(II) oxide, HgO), and the empirical formula of the second compound is \(Hg_2O_1\) (mercury(I) oxide, Hg_2O).

Step by step solution

01

Calculate the mass of oxygen in each compound

For both compounds, we need to calculate the mass of oxygen by using the initial mass of the compound and the mass of the remaining residue (for the first compound) or the mass loss (for the second compound). For the first compound: Mass of oxygen = Initial mass - Mass of residue For the second compound: Mass of oxygen = Mass loss
02

Convert mass of mercury and oxygen to moles

In order to find the mole ratio between mercury (Hg) and oxygen (O) in each compound, we first need to convert the mass of mercury and oxygen for each compound to moles. To do this, we divide the mass of the element by its molar mass. Molar mass of mercury (Hg) = 200.59 g/mol Molar mass of oxygen (O) = 16 g/mol For both compounds: Moles of mercury = Mass of mercury / Molar mass of mercury Moles of oxygen = Mass of oxygen / Molar mass of oxygen
03

Determine the mole ratio between mercury and oxygen in each compound.

To find the mole ratio of mercury (Hg) to oxygen (O) in each compound, divide the moles of mercury by the moles of oxygen. After that, try to simplify the ratios by dividing them with the greatest common divisor (GCD) if necessary. For both compounds: Mole ratio of Hg to O = Moles of mercury / Moles of oxygen
04

Determine the empirical formula of each compound

Once we have the mole ratio, we can write the empirical formula for each compound based on the ratio. The empirical formula for the first compound: Hg_xO_y (where x and y are the coefficients obtained from the mole ratio) The empirical formula for the second compound: Hg_aO_b (where a and b are the coefficients obtained from the mole ratio)

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Most popular questions from this chapter

Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing \(58 \% \mathrm{H}_{2} \mathrm{O}\) by mass is produced at the rate of \(1000 . \mathrm{kg} / \mathrm{h}\). What mass of water must be evaporated per hour if the final product contains only \(20 . \%\) water?

What amount (moles) is represented by each of these samples? a. \(20.0 \mathrm{mg}\) caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\) b. \(2.72 \times 10^{21}\) molecules of ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\) c. \(1.50 \mathrm{~g}\) of dry ice, \(\mathrm{CO}_{2}\)

Acrylonitrile \(\left(\mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}\right)\) is the starting material for many synthetic carpets and fabrics. It is produced by the following reaction. \(2 \mathrm{C}_{3} \mathrm{H}_{6}(g)+2 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{C}_{3} \mathrm{H}_{3} \mathrm{~N}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\) If \(15.0 \mathrm{~g} \mathrm{C}_{3} \mathrm{H}_{6}, 10.0 \mathrm{~g} \mathrm{O}_{2}\), and \(5.00 \mathrm{~g} \mathrm{NH}_{3}\) are reacted, what mass of acrylonitrile can be produced, assuming \(100 \%\) yield?

Elixirs such as Alka-Seltzer use the reaction of sodium bicarbonate with citric acid in aqueous solution to produce a fizz: \(3 \mathrm{NaHCO}_{3}(a q)+\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}(a q) \longrightarrow\) $$ 3 \mathrm{CO}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Na}_{3} \mathrm{C}_{6} \mathrm{H}_{3} \mathrm{O}_{7}(a q) $$ a. What mass of \(\mathrm{C}_{6} \mathrm{H}_{8} \mathrm{O}_{7}\) should be used for every \(1.0 \times 10^{2}\) \(\mathrm{mg} \mathrm{NaHCO}_{3} ?\) b. What mass of \(\mathrm{CO}_{2}(\mathrm{~g})\) could be produced from such a mixture?

A \(2.077-\mathrm{g}\) sample of an element, which has an atomic mass between 40 and 55, reacts with oxygen to form \(3.708 \mathrm{~g}\) of an oxide. Determine the formula of the oxide (and identify the element).
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