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3 years ago

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Another name for light is ________.

1 answer:

stich3 [128]3 years ago

5 0

Answer:

C &A

Explanation:

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One should know properties of constituents of a mixture to separate the mixture .Why?

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Answer:

Because: The mixtures contain unwanted substances which may be harmful and may degrade the properties of mixtures. So we, need to separated them and extract useful substances.

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3 years ago

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Suppose the reaction between nitrogen and hydrogen was run according to the amounts presented in Part A, and the temperature and

andrew11 [14]

Explanation:

Assuming that moles of nitrogen present are 0.227 and moles of hydrogen are 0.681. And, initially there are 0.908 moles of gas particles.

This means that, for $N_{2}(g) + 3H_{2}(g) \rightarrow 2NH_{3}$

moles of $N_{2}$ + moles of $H_{2}$ = 0.908 mol

Since, 2 moles of $N_{2}$ = $2 \times 0.227$ = 0.454 mol

As it is known that the ideal gas equation is PV = nRT

And, as the temperature and volume were kept constant, so we can write

$\frac{P(_in)}{n_(in)}$ = $\frac{P_(final)}{n_(final)}$

$\frac{10.4}{0.908}$ = $\frac{P_(final)}{0.454
}$

$P_(final)$ = $10.4 \times \frac{0.454}{0.908}$

= 5.2 atm

Therefore, we can conclude that the expected pressure after the reaction was completed is 5.2 atm.

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3 years ago

K12 3.10 Unit Assessment: Solutions, Part 1 does anyone have the answers for this quiz

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3 years ago

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Which do all cells need in order to function?

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Oxygen, should be correct
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3 years ago

The standard entropy of liquid methanol at 298K is 126.8 J/K-mol and its heat capacity is 81.6 J/K-mol. Methanol boils at 337K w

USPshnik [31]

Explanation:

First, we will calculate the entropies as follow.

$\Delta S_{2} = C_{p_{2}} ln \frac{T_{2}}{T_{1}}$ J/K mol

As, $T_{1}$ = 298 K, $T_{2}$ = 373.8 K

Putting the given values into the above formula we get,

$\Delta S_{2} = C_{p_{2}} ln \frac{T_{2}}{T_{1}}$ J/K mol

= $81.6 ln (\frac{373.8}{298})$

= 18.5 J/K mol

Now,

$\Delta S_{3} = \frac{\Delta H_{vap}}{T_{b.p}}$

= $\frac{35270 J}{373.8}$

= 94.2 J/mol K

Also,

$\Delta S_{4} = C_{p_{4}} ln \frac{T_{2}}{T_{1}}$

= $43.89 \times ln (\frac{800}{373.8})$

= 33.4 J/K mol

Now, we will calculate the entropy of one mole of methanol vapor at 800 K as follows.

$\Delta S_{T} = \Delta S^{o}_{1} + \Delta S_{2} + \Delta S_{3} + \Delta S_{4}$

= (126.8 + 18.5 + 94.2 + 33.4) J/K mol

= 272.9 J/K mol

Thus, we can conclude that the entropy of one mole of methanol vapor at 800 K is 272.9 J/K mol.

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3 years ago