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Gre4nikov [31]
2 years ago
13

Spell out full name of compound

Chemistry
2 answers:
andreyandreev [35.5K]2 years ago
8 0

Answer:

3-methyl-pentan-2-ol.

or

3-methyl-2-pentanol.

Explanation:

Hello,

In this case, such mocule is a branched alcohol since one commences numbering the chain by the right side of it, thus, we find a hydroxile and a methyl at the second and third carbons repectively. In this manner, the full name of the compound is:

3-methyl-pentan-2-ol.

or

3-methyl-2-pentanol.

As the main functional group is the hydroxide which characterizes the compound as an alcohol.

Best regards.

Margarita [4]2 years ago
7 0
Hydroxide is the full name of the compound.

Hope this Helped!

;D
Brainliest??
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miskamm [114]

<u>Answer:</u> The \Delta H^o_{rxn} for the reaction is -1835 kJ.

<u>Explanation:</u>

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

P_4(g)+10Cl_2(g)\rightarrow 4PCl_5(s)      \Delta H^o_{rxn}=?

The intermediate balanced chemical reaction are:

(1) PCl_5(s)\rightarrow PCl_3(g)+Cl_2(g)    \Delta H_1=157kJ   ( × 4)

(2) P_4(g)+6Cl_2(g)\rightarrow 4PCl_3(g)     \Delta H_2=-1207kJ

The expression for enthalpy of the reaction follows:

\Delta H^o_{rxn}=[4\times (-\Delta H_1)]+[1\times \Delta H_2]

Putting values in above equation, we get:

\Delta H^o_{rxn}=[(4\times (-157))+(1\times (-1207))=-1835kJ

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Answer:

This is a pretty straightforward example of how an ideal gas law problem looks like.

Your strategy here will be to use the ideal gas law to find the pressure of the gas, but not before making sure that the units given to you match those used by the universal gas constant.

So, the ideal gas law equation looks like this

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

P

V

=

n

R

T

a

a

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∣

−−−−−−−−−−−−−−−

Here you have

P

- the pressure of the gas

V

- the volume it occupies

n

- the number of moles of gas

R

- the universal gas constant, usually given as

0.0821

atm

⋅

L

mol

⋅

K

T

- the absolute temperature of the gas

Take a look at the units given to you for the volume and temperature of the gas and compare them with the ones used in the expression of

R

.

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Liters, L

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Liters, L

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Kelvin, K

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Celsius,

∘

C

a

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×

Notice that the temperature of the gas must be expressed in Kelvin in order to work, so make sure that you convert it before plugging it into the ideal gas law equation

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

T

[

K

]

=

t

[

∘

C

]

+

273.15

a

a

∣

∣

−−−−−−−−−−−−−−−−−−−−−−−−

Rearrange the ideal gas law equation to solve for

P

P

V

=

n

R

T

⇒

P

=

n

R

T

V

Plug in your values to find

P

=

0.325

moles

⋅

0.0821

atm

⋅

L

mol

⋅

K

⋅

(

35

+

273.15

)

K

4.08

L

P

=

∣

∣

∣

∣

¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯

a

a

2.0 atm

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The answer is rounded to two sig figs, the number of sig figs you have for the temperature of the gas.

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