Balance the following redox reaction in acidic solution?
#\sf{P_4(s)+NO_3^(-)\toH_2PO_4^(-)(aq)+NO(g)}#
I have the oxidation, but not the reduction.
Answer key tells me there is #\tt{2H_2O}# but that doesn't match with the #\tt{NO_3^(-)}# on the other end of the arror.
Plus, why add #\tt{3e^-}# ? Bounded oxygen typically has a charge of -2, right? So three oxygens equals six electrons...?
I have the oxidation, but not the reduction.
Answer key tells me there is
Plus, why add
And so elemental phosphorus
Since the mass and charge are balanced, this is kosher.
...and proceed to cancel...
Since anyone can manipulate the arifmetik, is this balanced? If not, should it be? We know that an unbalanced representation of mass and charge cannot be taken seriously as accurate depiction of reality.
Phosphorus and nitrogen alone are involved in redox in this situation; oxygen is not. In reality, all I have done is assign oxidation states.
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Final balanced equation:
Let's get started:
I can carefully insert water and hydrogen ions wherever they are needed in the equation when it is in an acidic solution:
Each side's electrons must be equal:
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Please provide the redox reaction that you would like me to balance in acidic solution.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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