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Solnce55 [7]
2 years ago
5

Combustion Analysis of an unknown hydrocarbon resulted in the capture of 216.00 g of water vapor and 440.00 g of CO2. The total

mass of the hydrocarbon before combustion was 144 g.
(1. How many moles of carbon dioxide are present after combustion?)

(2. What is the empirical formula for the unknown hydrocarbon?)

(3. How many water molecules does the water vapor trap capture?)

(4. The gram-formula mass for the unknown hydrocarbon was determined to be 72 g/mol. How many moles of the unknown hydrocarbon were present in the original sample?)

(5. infrared spectral analysis determines that the unknown hydrocarbon does NOT contain oxygen. How many moles of O2 are used in combusting the unknown sample?)
Chemistry
1 answer:
LenKa [72]2 years ago
4 0

1: 10 mol CO2

2: C10H24

3: 12 mol H2O

4: 0.5 mol

5: 16 mol O2

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See explanation

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Electron affinity is the energy released when an extra electron is added to a neutral gaseous atom. A negative value of electron affinity indicates that energy is given out and vice versa.

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2 years ago
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8 0
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A solution is made containing 4.6 g of sodium chloride per 250g of water.
lozanna [386]

Answer:

\large \boxed{1.81 \, \%}

Explanation:

\text{Mass percent} = \dfrac{\text{mass of solute} }{\text{mass of solution}} \times 100 \, \%

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Mass of NaCl =      4.6 g

Mass of water = 250    g

Calculations:

Mass of solution = mass of NaCl + mass of water = 4.6 g + 250 g = 254.6 g.

\text{\% m/m} = \dfrac{\text{4.6 g} }{\text{254.6 g}} \times 100 \, \% = \mathbf{1.81 \, \%}\\\\\text{The percent by mass of NaCl is $\large \boxed{\mathbf{1.81 \, \%}}$}

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