The calculation is (Measurement in m³ x 1000³)

Therefore

Measurement in m³ x 1 000 000

Its not a fraction as there are 1000mm in a m, so to convert from m to mm you must multiply

5 0

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.

7 0

3 years ago

How many moles are in a 4.5g of Sulfur?

Vadim26 [7]

Answer:

~0.14

Explanation:

There are roughly ~0.14 moles in 4.5g of Sulfur. 1 mol = 32.06 g of Sulfur, so we just find the ratio and then multiply.

5 0

3 years ago

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