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3 years ago

Which of the following is not a organic compound, a -corn oil b -b r o m i n e c -m e t h a n e d- protein

2 answers:

6 0

A corn oil. Because oil is treated with a solvent. After that it is refined which gets rid of free fatty acids. Finally, it is sent through steam distillation to get rid of volatile organic compounds.

madreJ [45]3 years ago

5 0

The correct answer to your question is... A corn oil.

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9. A gas occupies 8.2 L at 48°C and 750. torr. What volume will the gas occupy at STP?

slava [35]

Answer: The volume the gas will occupy at STP is 6.9 L

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law.

The combined gas equation is,

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1$ = initial pressure of gas = 750 torr = 0.99 atm (760torr=1atm)

$P_2$ = final pressure of gas = 1 atm (at STP)

$V_1$ = initial volume of gas = 8.2 L

$V_2$ = final volume of gas = ?

$T_1$ = initial temperature of gas = $48^oC=273+48=321K$

$T_2$ = final temperature of gas = $273K$ (at STP)

Now put all the given values in the above equation, we get:

$\frac{0.99\times 8.2}{321}=\frac{1\times V_2}{273}$

$V_2=6.9$

Thus volume the gas will occupy at STP is 6.9 L

7 0

3 years ago

How many grams of H2S is needed to produce 18.00g of PbS if the H2S is reacted with an

goldenfox [79]

Answer:

2.56 grams of H₂S is needed to produce 18.00g of PbS if the H2S is reacted with an excess (unlimited) supply of Pb(CH₃COO)₂

Explanation:

The balanced reaction is:

Pb(CH₃COO)₂ + H₂S → 2 CH₃COOH + PbS

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction) they react and produce:

Pb(CH₃COO)₂: 1 mole
H₂S: 1 mole
CH₃COOH: 2 moles
PbS: 1 mole

In this case, to know how many grams of H₂S are needed to produce 18.00 g of PbS, it is first necessary to know the molar mass of the compounds H₂S and PbS and then to know how much it reacts by stoichiometry. Being:

H: 1 g/mole
S: 32 g/mole
Pb: 207 g/mole

The molar mass of the compounds are:

H₂S: 2* 1 g/mole + 32 g/mole= 34 g/mole
PbS: 207 g/mole + 32 g/mole= 239 g/mole

So, by stoichiometry they react and are produced:

H₂S: 1 mole* 34 g/mole= 34 g
PbS: 1 mole* 239 g/mole= 239 g

Then the following rule of three can be applied: if 239 grams of PbS are produced by stoichiometry from 34 grams of H₂S, 18 grams of PbS from how much mass of H₂S is produced?

$mass of H_{2} S=\frac{18 grams of PbS*34 grams of H_{2}S }{239 grams of PbS}$

mass of H₂S= 2.56 grams

<u><em>2.56 grams of H₂S is needed to produce 18.00g of PbS if the H2S is reacted with an excess (unlimited) supply of Pb(CH₃COO)₂</em></u>

8 0

3 years ago

Select all the correct locations on the image.

gavmur [86]

Answer:

I think the correct answer is f

6 0

3 years ago

26. Classify each chemical equation as a combination/synthesis , decomposition, single replacement, double replacement, or combu

Natali [406]

These are the answers.

8 0

2 years ago

A sample of carbon dioxide gas (CO2) contains 8.551 x 1025 molecules. How many moles of carbon dioxide does this represent?

ozzi

Answer:

142.0 moles CO₂

Explanation:

To answer this question, we first need to know what a mole is. A mole represents $6.022 \cdot 10^{23}$ of something, and in this case, that something is molecules.

So, to convert $8.551 \cdot 10^{25}$ molecules into moles, we need to use the conversion factor $1=\frac{6.022\cdot 10^{23} \text{molecules} }{ \text{1 mole}}$ .

Doing so (using dimensional analysis) gives us:

$8.551 \cdot 10^{25} \text{ molecules } \cdot \frac{\text{1 mole}}{ 6.022\cdot 10^{23} \text{ molecules} } = \frac{8.551 \cdot 10^{25}}{ 6.022\cdot 10^{23}} \text{ moles CO}_2 = \\ \\ 141.996 \text{ moles CO}_2 = \boxed{142.0 \text{ moles CO}_2 }$

8 0

3 years ago