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FromTheMoon [43]
3 years ago
12

A compound contains only carbon, hydrogen, and oxygen. Combustion of 10.68mg of the compound yields 16.01 mg CO2 and 4.37 mg H2O

. The molar mass of the compound is 176.1g/mol. What are the empirical and molecular formulas?
Chemistry
1 answer:
Zielflug [23.3K]3 years ago
6 0
<span>Molecular formulas tell you how many atoms of each element are in a compound, and empirical formulastell you the simplest or most reduced ratio of elements in a compound. ... Also, many compounds with different molecular formula have the same<span>empirical formula</span></span>
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A commercial oven with a book value of $67,000 has an estimated remaining 5 year life. A proposal is offered to sell the oven fo
baherus [9]

Answer:

$13,500

Explanation:

The differential analysis of the proposal to replace the commercial oven is shown below:-  

The Total differential decrease in cost = Annual maintenance cost reduction × Number of years applicable

= $23,000 × 5

= $115,000  

Inflow cash = The Total differential decrease in cost + Proceeds from sale of equipment

= 115,000 + $8,500

= $123,500

The Net differential decrease in cost from replacing equipment = Inflow cash - Cost of new equipment

= $123,500 - $110,000

= $13,500

8 0
2 years ago
Propose the structure of the following HNMR data.
Varvara68 [4.7K]

Answer:

1-Chloropropane is likely the answer (attached a picture)

Explanation:

First off there are 3 peaks and 3 carbons which indicates to me that this will be a chain without any symmetry and that each carbon has hydrogens on it.  

Second the triplet at 1.0 that integrates to 3 likely correlates to a CH3 (methyl) group.  Peaks are very upfield triplets that integrate to three are almost always methyl peaks.

Third the triplet at 3.7 is indicative of being next to the halogen.  Hydrocarbons by themselves do not have peaks that far downfield meaning that its shift could only be explained by the chlorine being involved.  Also we know that this can't be next to the methyl group since its multiplicity is to low to be next to it.  

That leaves the multiplet at 1.75 being the hydrogens on the middle carbon which also makes sense since it is more downfield then the methyl group (due to being closer to the chlorine) but is not far enough downfield to say the chlorine is there.  It also makes sense that it is a multiple since it would be a hextet due to the adjacent 5 hydrogens which can't always be resolved.

I hope this helps and let me know if anything is unclear or needs further explanation.

7 0
2 years ago
Which of the following is an example of a compound?<br> H2O<br> Na<br> Cl<br> O
andrezito [222]
H2O
The other ones are just elements
3 0
2 years ago
1. Calculate the concentration of hydronium ion of both buffer solutions at their starting pHs. Calculate the moles of hydronium
lilavasa [31]

Answer:

This question is incomplete, here's the complete question:

1. Calculate the concentration of hydronium ion of both buffer solutions at their starting pHs. Calculate the moles of hydronium ion present in 20.0 mL of each buffer.

Buffer A

Mass of sodium acetate used: 0.3730 g

Actual ph of the buffer 5.27

volume of the buffer used in buffer capacity titration 20.0 mL

Concentration of standardized NaOH 0.100M

moles of Naoh needed to change the ph by 1 unit for the buffer 0.00095mol

the buffer capacity 0.0475 M

Buffer B

Mass of sodium acetate used 1.12 g

Actual pH of the buffer 5.34

Volume of the buffer used in buffer capacity titration 20.0 mL

Concentration if standardized NaOH 0.100 M

moles of Naoh needed to change the ph by 1 unit 0.0019 mol

the buffer capacity 0.095 M

2.) A change of pH by 1 unit means a change in hydronium ion concentration by a factor of 10. Calculate the number of moles of NaOH that would theoretically be needed to decrease the moles of hydronium you calculated in #1 by a factor of 10 for each buffer. Are there any differences between your experimental results and the theoretical calculation?

3.) which buffer had a higher buffer capacity? Why?

Explanation:

Formula,

moles = grams/molar mass

molarity = moles/L of solution

1. Buffer A

molarity of NaC2H3O2 = 0.3731 g/82.03 g/mol x 0.02 L = 0.23 M

molarity of HC2H3O2 = 0. 1 M

Initial pH

pH = pKa + log(base/acid)

= 4.74 + log(0.23/0.1)

= 5.10

pH = -log[H3O+]

[H3O+] = 7.91 x 10^-6 M

In 20 ml buffer,

moles of H3O+ = 7.91 x 10^-6 M x 0.02 L

= 1.58 x 10^-7 mol

Buffer B

molarity of NaC2H3O2 = 1.12 g/82.03 g/mol x 0.02 L = 0.68 M

molarity of HC2H3O2 = 0.3 M

Initial pH

pH = pKa + log(base/acid)

= 4.74 + log(0.68/0.3)

= 5.10

pH = -log[H3O+]

[H3O+] = 7.91 x 10^-6 M

In 20 ml buffer,

moles of H3O+ = 7.91 x 10^-6 M x 0.02 L

= 1.58 x 10^-7 mol

2. let x moles of NaOH is added,

Buffer A,

pH = 5.10

[H3O+] = 7.91 x 10^-6 M

new pH = 4.10

new [H3O+] = 7.91 x 10^-5 M

moles of NaOH to be added = (7.91 x 10^-5 - 7.91 x 10^-6) x 0.02 L

= 1.42 x 10^-6 mol

3. Buffer B with greater concentration of NaC2H3O2 and HC2H3O2 has higher buffer capacity as it resists pH change to a wider range due to addition of acid or base to the system as compared to low concentration of Buffer A

5 0
3 years ago
Calculate ΔrG∘ at 298 K for the following reactions.CO(g)+H2O(g)→H2(g)+CO2(g)2-Predict the effect on ΔrG∘ of lowering the temper
KonstantinChe [14]

Answer:

1) ΔG°r(298 K) = - 28.619 KJ/mol

2) ΔG°r will decrease with decreasing temperature

Explanation:

  • CO(g) + H2O(g) → H2(g) + CO2(g)

1) ΔG°r = ∑νiΔG°f,i

⇒ ΔG°r(298 K) = ΔG°CO2(g) + ΔG°H2(g) - ΔG°H2O(g) - ΔG°CO(g)

from literature, T = 298 K:

∴ ΔG°CO2(g) = - 394.359 KJ/mol

∴ ΔG°CO(g) = - 137.152 KJ/mol

∴ ΔG°H2(g) = 0 KJ/mol........pure substance

∴ ΔG°H2O(g) = - 228.588 KJ/mol

⇒ ΔG°r(298 K) = - 394.359 KJ/mol + 0 KJ/mol - ( - 228.588 KJ/mol ) - ( - 137.152 KJ7mol )

⇒ ΔG°r(298 K) = - 28.619 KJ/mol

2) K = e∧(-ΔG°/RT)

∴ R = 8.314 E-3 KJ/K.mol

∴ T = 298 K

⇒ K = e∧(-28.619/(8.314 E-3)(298) = 9.624 E-6

⇒ ΔG°r = - RTLnK

If T (↓) ⇒ ΔG°r (↓)

assuming T = 200 K

⇒ ΔG°r(200 K) = - (8.314 E-3)(200)Ln(9.624E-3)

⇒ ΔG°r (200K) = - 19.207 KJ/mol < ΔG°r(298 K) = - 28.619 KJ/mol

6 0
3 years ago
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