Respuesta :
Answer:
The answer to your question is: 0.015 mole of NO
Explanation:
Data
Silver = Ag = 0.1 mole
Nitric acid = HNO3 = 10 ml 6 M
Balanced reaction
3Ag + 4HNO₃ ⇒ 3AgNO₃ + NO + 2H₂O
# moles of HNO₃ = 6(0.01) = 0.06
Limiting reactant HNO₃ because for the amount of silver given
the reaction needs 0.133 moles of acid, and there
are only 0.06
4 mol of HNO₃ ------------------- 1 mol of NO
0.06 mol of Ag ------------------ x
x = (0.06 x 1) / 4
x = 0.015 mol
The moles of NO formed from the given reaction has been 0.015 mol. Thus, option A is correct.
The balanced chemical equation for the reaction has been:
[tex]\rm 3\;Ag\;+\;4\;HNO_3\;\rightarrow\;3\;AgNO_3\;+\;NO\;+\;2\;H_2O[/tex]
The moles of nitric acid can be given as:
Moles = Molarity × Volume
The molarity of nitric acid = 6 M
Volume of nitric acid = 10 ml = 0.01 L
Moles of nitric acid = 6 × 0.01 mol
Moles of nitric acid = 0.06 mol.
From the balanced equation,
3 moles silver requires = 4 moles nitric acid
0.10 moles silver requires = [tex]\rm \dfrac{4}{3}\;\times\;0.10[/tex] moles nitric acid
0.10 moles silver requires = 0.13 mol nitric acid.
Since the available nitric acid is 0.06 mol, it has been in lesser amount and has been the limiting reagent.
Thus,
4 moles nitric acid = 1 moles NO
0.06 mol nitric acid = 0.015 moles NO.
Thus, the moles of NO formed from the given reaction has been 0.015 mol. Thus, option A is correct.
For more information about the moles in a equation, refer to the link:
https://brainly.com/question/16208222
