Please can you solve completely? Because when I solved I didn't get any option in 2nd part question.This is a question about balancing the chemical reactions, which relate moles of reactants and products, using the measured masses of both.
So start by calculating what you know from the information given. How can you get the grams and moles of the gas produced, given the volume? Once you know the moles of gas, what does that tell you about the rest of the reactions?
We will NOT work your homework for you. It is YOUR homework.But I want answer only for 2nd question. Please can you solve it? I am having problem in that only.
Same answer as before in #4: Show where you're stuck. If you've balanced the equations and done enough work to answer the first part, this second part should be easy. I suspect you're just not seeing the simple solution right in front of you.But I want answer only for 2nd question. Please can you solve it? I am having problem in that only.
You’ve neglected the consumption of acid by the zinc reaction. Notice how the question was constructed to slightly obscure the involvement of HNO3 in that rxn.This way I am getting 14.16 ml but not an accurate answer.
Please help me to get correct answer.
I finally got around to looking at the calculations and now I see your dilemma. 2 grams of brass, even if it’s pure copper, is only 0.0315 moles and yet it appears that 0.0425 miles of NO2 were produced. Something is wrong here but I’m not seeing it.If I include the reaction with Zn also volume will come more than 16 ml.
The equations clearly are not balanced. Just look at the number of hydrogen atoms on both sides of each one.Perhaps the equations are not really balanced? Note: Cu (II) needs a geganion (anion). Maybe the student was expected to do the redox calculations to balance them.
That is not what I said, nor would anyone who knows how to work REDOX equations interpret it that way. I have never seen anyone approach such problems by balancing "hydrogen atoms" (H· ) to balance the oxidation/reduction states. Sure, there has to be elemental balance, but that is not always sufficient.So the atoms don't have to be balanced, just the electrons....???
The post I was responding to seemed to not be sure whether they were balanced or not (as indicted by "perhaps the equations are not really balanced"). So I was trying to point out that a casual glance at the equations show that they are not balanced -- it doesn't matter which particular atom is not balanced, if ANY atom is not balanced on left and right, then the equation is not balanced. In the case of both of these equations, it is seemed (to me) trivial to note that the hydrogen atoms are not balanced and therefore I commented that "clearly they are not balanced". That assertion was not in any way based on ANY implication that balancing hydrogen atoms is a SUFFICIENT condition to balance the oxi/redux states, only that it is a NECESSARY condition.That is not what I said, nor would anyone who knows how to work REDOX equations interpret it that way. I have never seen anyone approach such problems by balancing "hydrogen atoms" (H· ) to balance the oxidation/reduction states. Sure, there has to be elemental balance, but that is not always sufficient.
Nevertheless, I have learned from experience not to get drawn into a trivial, off-topic disagreement with you and will not contribute to this thread further. I do hope the TS takes my advice, writes the half equations, and balances the electronic states. The rest will fall into place from those equations.
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