N2 + 3 H2 – 2 NH3 How many moles of nitrogen (N2) are required to get 6
1 answer:
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Explanation:
The reaction equation will be as follows.
Hence, the expression for is as follows.
Let us assume that the concentration of both and
is x.
x = 0.01118034
This means that the concentration of is 0.01118034.
Since, we know that the relation between pH and concentration of hydrogen ions is as follows.
pH =
=
= 1.958
Thus, we can conclude that the pH of a 0.500 M solution of arsenic acid is 1.958.
Answer:
B
Explanation:
This question is about stoichiometry. From the balanced equation ⇒
, we see that 3 moles of water is needed to react with 1 mole of
.
This means that, to fully react 3.62 moles of , we would need 3*3.62 or 10.86 moles of water. However, we only have 6.31 moles, so water is the limiting reactant.
Since 3 moles of water react with 1 mole of , 6.31 moles of water can fully react with 6.31÷3 or 2.1033 moles of
.
From the balanced equation, we see that every mole of reacted gets you 2 moles of
. Therefore, 2.1033 moles of
would give you approximately 4.21 moles of
.