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Below is a balanced equation for the reaction of nitrogen with hydrogen to produce ammonia.

Which conversion factor(s) would be used if the mass (in g) of hydrogen were given and it needed to be converted to moles?

$$N_{2}(g)\ +\ 3H_{2}(g)\rightarrow 2NH_{3}(g)$$

Select ALL that apply.

A

$\cfrac{2.0159\ g\ H_{2}}{1\ \text{mole}}$

B

$\cfrac{1\ \text{mole}}{2.0159\ g\ H_{2}}$

C

$\cfrac{17.0337\ g\ NH_{3}}{1\ \text{mole}}$

D

$\cfrac{1\ \text{mole}}{17.0337\ g\ NH_{3}}$

E

$\cfrac{6.022\times 10^{23}\ \text{molecules}}{1\ \text{mole}}$

F

$\cfrac{1\ \text{mole}}{6.022\times 10^{23}\ \text{molecules}}$

G

$\cfrac{2\ \text{mole} \ NH_{3}}{3\ \text{mole} \ H_{2}}$

H

$\cfrac{3\ \text{mole} \ H_{2}}{2\ \text{mole} \ NH_{3}}$

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