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svetoff [14.1K]
3 years ago
8

A compound is found to contain 64.80% carbon. 13.62% hydrogen. And 21.58% oxygen by weight. What is the empirical formula for th

is compound?
Show all your work

Chemistry
2 answers:
Trava [24]3 years ago
7 0

Answer:

Look at sheet

Explanation:

Ight so like I'm too lazy to type this out just look at my work. Idk why it works I just know it works

oksano4ka [1.4K]3 years ago
6 0

Answer: C4H10O

Explanation: First identify the number of moles on each atom by having the relationship of 1 mole = molar mass

Second step is to divide the lowest amount to each atom.

Third the answer will be the number of individual atoms on each element in the empirical formula.

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Alice and Bob are experimenting with two moles of neon, a monatomic gas, that starts out at conditions of standard temperature a
Archy [21]

Answer:

29273.178 joules have been added to the gas for the entire process.

Explanation:

The specific heats of monoatomic gases, measured in joules per mol-Kelvin, are represented by the following expressions:

Isochoric (Constant volume)

c_{v} = \frac{3}{2}\cdot R_{u} (1)

Isobaric (Constant pressure)

c_{p} = \frac{5}{2}\cdot R_{u} (2)

Where R_{u} is the ideal gas constant, measured in pascal-cubic meters per mol-Kelvin.

Under the assumption of ideal gas, we notice the following relationships:

1) Temperature is directly proportional to pressure.

2) Temperature is directly proportional to volume.

Now we proceed to find all required temperatures below:

(i) <em>Alice heats the gas at constant volume until its pressure is doubled</em>:

\frac{T_{2}}{T_{1}} = \frac{P_{2}}{P_{1}} (3)

(\frac{P_{2}}{P_{1}} = 2, T_{1} = 273.15\,K)

T_{2} = \frac{P_{2}}{P_{1}} \times T_{1}

T_{2} = 2\times 273.15\,K

T_{2} = 546.3\,K

(ii) <em>Bob further heats the gas at constant pressure until its volume is doubled</em>:

\frac{T_{3}}{T_{2}} =\frac{V_{3}}{V_{2}} (4)

(\frac{V_{3}}{V_{2}} = 2, T_{2} = 546.3\,K)

T_{3} = \frac{V_{3}}{V_{2}}\times T_{2}

T_{3} = 2\times 546.3\,K

T_{3} = 1092.6\,K

Finally, the heat added to the gas (Q), measured in joules, for the entire process is:

Q = n\cdot [c_{v}\cdot (T_{2}-T_{1})+c_{p}\cdot (T_{3}-T_{2})] (5)

If we know that R_{u} = 8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K}, n = 2\,mol, T_{1} = 273.15\,K, T_{2} = 546.3\,K and T_{3} = 1092.6\,K, the heat added to the gas for the entire process is:

c_{v} = \frac{3}{2}\cdot \left(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} \right)

c_{v} = 12.471\,\frac{J}{mol\cdot K}

c_{p} = \frac{5}{2}\cdot \left(8.314\,\frac{Pa\cdot m^{3}}{mol\cdot K} \right)

c_{p} = 20.785\,\frac{J}{mol\cdot K}

Q = (2\,mol)\cdot \left[\left(12.471\,\frac{J}{mol\cdot K} \right)\cdot (536.3\,K-273.15\,K)+\left(20.785\,\frac{J}{mol\cdot K} \right)\cdot (1092.6\,K-546.3\,K )\right]

Q = 29273.178\,J

29273.178 joules have been added to the gas for the entire process.

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Answer:

We need more detail

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Explanation:

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Answer:

Ethane & propane are members of same homologous series : alkane which is indicated with Cn H2n+2

Explanation:

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Explanation:

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