Solving Chemistry Problem: As + HNO3 -> H3AsNO4 + NO2 + H2O

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In summary, the conversation is about balancing the equation for the reaction between + HNO3 (consentrated) and H3AsNO4, NO2, and H2O. The attempt at a solution involved calculating the oxidation numbers and balancing the sides, but there was confusion about the formula of H3AsNO4 and the oxidation numbers. The conversation ends with the conclusion that the equation may not be balanced due to incorrect formula and the difficulty in determining the oxidation numbers.
  • #1
fawk3s
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Homework Statement



As + HNO3 (consentrated) -> H3AsNO4 + NO2 + H2O

Homework Equations



none

The Attempt at a Solution



I tried doing the electron equation:

As (0) - 1 electron = As (1+) | 1
N (5+) + 1 electron = N (4+) | 1

I don't know if this is right. (The last 2 numbers are supposed to represent the numbers which should go in the equation before those elements.)
Think the oxydation level is supposed to change, but the sides don't balance out. What am I doing wrong? I just can't get this out of my head anymore.

Thanks in advance,
fawk3s
 
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  • #2
What is formula of your As containing product? Seems to me something is wrong with the way you wrote it in the equation. What is ON of As after oxidation?

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  • #3
Borek said:
What is formula of your As containing product? Seems to me something is wrong with the way you wrote it in the equation. What is ON of As after oxidation?

Im not sure actually. The equation was given like that and I am not even sure what the oxydation levels are supposed to be.
My task was only to balance the sides.
 
  • #5
Borek said:
As far as I can tell formula of H3AsNO4 is wrong (no such compound) and equation can be not balanced.

Oxidation numbers you can easily calculate following simple rules.

Yeah, that would explain why I can't figure it out still after trying for an hour or so.

And yes, I know how to calculate the oxidation numbers, but if the oxidaton number of N didnt change during the reaction, then As has to be 0. And that would be odd.

Anyways, thanks for the help !
 

FAQ: Solving Chemistry Problem: As + HNO3 -> H3AsNO4 + NO2 + H2O

How do I balance this chemical equation?

To balance a chemical equation, you must ensure that there is an equal number of atoms of each element on both sides of the equation. Start by counting the number of atoms for each element on each side, and then use coefficients to balance the equation. In this case, you would need two molecules of HNO3 and three molecules of H3AsNO4 to balance the equation.

What is the role of each reactant and product in this equation?

The reactants in this equation are As and HNO3. As is a solid element and HNO3 is a liquid compound. They react together to form the products H3AsNO4, NO2, and H2O. H3AsNO4 is the main product and is a solid compound, while NO2 and H2O are gaseous products.

How do I determine the limiting reagent in this reaction?

To determine the limiting reagent, you must first calculate the moles of each reactant present using their respective molar masses. Then, compare the moles of each reactant to the stoichiometric ratio in the balanced equation. The reactant with the smaller number of moles is the limiting reagent, as it will be completely consumed in the reaction and limit the amount of product that can be formed.

What is the oxidation state of As in the product H3AsNO4?

The oxidation state of As in H3AsNO4 is +5. This can be determined by assigning oxidation states to all the other elements in the compound (H=+1, N=+5, O=-2) and using the fact that the sum of all oxidation states in a compound must equal the overall charge, which in this case is 0.

How can I tell if this reaction is exothermic or endothermic?

This reaction is exothermic because it releases heat. This can be determined by looking at the enthalpy (ΔH) of the reaction, which is negative for exothermic reactions. In this case, the ΔH is -136.6 kJ/mol, indicating that the reaction is exothermic.

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