Nuclear charge from a potential electrostatic energy

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Discussion Overview

The discussion revolves around calculating the nuclear charge from a given electrostatic potential energy and distance, as well as addressing related homework questions on molar mass and redox reactions. The scope includes theoretical calculations, homework-related queries, and conceptual clarifications.

Discussion Character

  • Homework-related
  • Conceptual clarification
  • Technical explanation

Main Points Raised

  • One participant presents a calculation for nuclear charge using the formula for electrostatic potential energy but expresses confusion about whether the calculated charge represents the nuclear charge and the implications of the sign of the charge.
  • Another participant questions the accuracy of the molar mass of Mo(CO)6, seeking confirmation from others.
  • A participant mentions receiving a wrong mark for the molar mass question and speculates that it may relate to significant figures or calculation errors.
  • Another participant expresses difficulty with a homework question regarding redox reactions, attempting to identify which element is oxidized and which is reduced, and provides a chemical equation for context.
  • The participant proposes that Iron is oxidized due to the loss of electrons but is uncertain about which species is reduced, initially guessing sulfate but later considering sulfur.

Areas of Agreement / Disagreement

Participants do not appear to reach consensus on the nuclear charge calculation or the redox reaction question. There are multiple competing views and uncertainties expressed regarding the calculations and interpretations of the homework problems.

Contextual Notes

Participants express uncertainty about the implications of signs in charge calculations and significant figures in their answers. There is also a lack of clarity on the correct identification of oxidized and reduced species in the redox reaction.

Who May Find This Useful

Students working on electrostatics, redox reactions, and molar mass calculations may find this discussion relevant.

RJLiberator
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Question: "Given an electrostatic potential energy of -6.16x10^-18 J and a distance of 1.12x10^-10m, what is the nuclear charge if there is a single electron interacting with the nucleus?"

Okay, Equation:
PE = [K*Q1*Q2]/d

Where K is a constant of 8.99*10^9 J*m/c
d is giving at 1.12*10^-10m
PE is giving at -6.16*10^-18 J
Q1 is giving as the charge of an electron at 1.602 * 10^-19 C
Q2 is what we solve for, which, plugging in the equation is -4.79*10^-19

This equation is easy enough to plug in. HOWEVER, am I answering the equation? Is Q2 = to the nuclear charge? I guess that is where I am confused.

And for Q2 I received a negative charge, I would imagine this is correct since PE is initially negative and the charge of an electron was positive? Or do I have it backwards?

Thank you
 
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I just realized I may have posted this with the worst possible title of a thread. I apologize.

Can anyone confirm that the MOLAR MASS of Mo(CO)6 is 264.0 ?
 
RJLiberator said:
I just realized I may have posted this with the worst possible title of a thread. I apologize.

Can anyone confirm that the MOLAR MASS of Mo(CO)6 is 264.0 ?

Yep, looks OK.
 
Interesting. I got that answer marked wrong on the online application. It must be due to the amount of figures, however the question explicitly states to go to one decimal point on all of these questions. I will e-mail my professor before going through my second attempt.

Anyone have any idea on the first one? I got it marked incorrectly and I am not sure if its because of the sign, significant figures or error in calculation.
 
Sorry for posting all of my junk here. However, I am having the most difficulty with this homework. I want to understand, but I feel like I am missing an integral piece. Anyway, I will keep treading on. Here is my next question.

"For the reaction between Iron and sulfuric acid, which element is reduced?" And which is oxidized?
a) Iron
b) Hydrogen
c) Sulfur

Okay. Well, the equation should be

2Fe (s) + 3H2SO4 (aq) ---> Fe2(SO4)3 (aq) + 3H2 (g)

Oxidization refers to loss of electrons in the reaction. Reduction is the gain of electrons.

Well naturally, Iron will look to loss electrons. So that would make it the obvious choice to be oxidized.
However, who gains electrons? My initial guess is "Sulfate." However, that is not an option. I attempted with oxygen previously and it was incorrect. So it must be Sulfur?
 

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