Easy Stoichiometry Concentration Problem

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Discussion Overview

The discussion revolves around stoichiometry problems involving reactions between iron and copper(II) sulfate, as well as zinc and hydrochloric acid. Participants are attempting to calculate the minimum volume of copper(II) sulfate solution required based on the mass of copper precipitated and to determine the mass of hydrogen gas generated from a reaction with zinc.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Technical explanation
  • Debate/contested

Main Points Raised

  • One participant presents a calculation involving the mass of copper precipitated and attempts to derive the volume of copper(II) sulfate solution needed, expressing uncertainty about their approach.
  • Another participant questions the validity of the calculations, specifically the number of moles and the resulting volume, suggesting that the notation used is problematic.
  • There is a discussion about the molecular mass of hydrogen, with one participant noting that hydrogen is diatomic and providing its correct molecular mass as 2.02 amu.
  • A later post prompts further inquiry into the number of moles of copper produced and the corresponding moles of copper sulfate required for the reaction.

Areas of Agreement / Disagreement

Participants do not appear to reach a consensus on the calculations presented, with multiple viewpoints on the correct approach and results. Uncertainty remains regarding the initial calculations and the interpretation of stoichiometric relationships.

Contextual Notes

Participants express confusion over the calculations and notation used, indicating potential misunderstandings of stoichiometric principles and the relationships between reactants and products. There are unresolved steps in the calculations presented.

Who May Find This Useful

This discussion may be useful for students learning stoichiometry, particularly in understanding how to approach problems involving chemical reactions and the calculations of reactants and products.

htrrht
Messages
2
Reaction score
0
1. A piece of iron was added to a beaker that contained 0.585 mol/L copper(II) sulfate, CuSO4(aq). The solid copper that precipitated was dried, and its mass was found to be 5.02 g. Some unreacted iron remained in the beaker. Calculate the minimum volume of the copper(II) sulfate solution.

I really have no idea what I'm doing, seriously. I pretty much just guessed and my answer is almost guaranteed to be completely wrong.

This is what I have:

0.585mol CuSO4 / 1 L = 1 mol Cu / 1 mol CuSO4 = x / 5.02g Cu = 5.02g CuSO4
n=5.02g CuSO4 / 159.62 g/mol = 0.031 mol CuSO4
v = 0.585mol / L / 0.031 mol
v = 18.4 L.

2. To generate hydrogen gas, a teacher added 25.0 g of mossy zinc to 220 mL of 3.00 mol/L hydrochloric acid in an Erlenmeyer flask.

a. What mass of hydrogen gas was generated?

b. Aft er the reaction, what was the concentration of zinc chloride, ZnCl2(aq), in the fl ask?

Again I honestly have no idea what to do for this problem, I don't even know how to start...
 
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One step at a time: mixing "run-on" notation with conventional notation is a no-no. 0.031 moles? Maybe. 18.4 l? No.

What's the "molecular mass" for hydrogen?
 
Bystander said:
One step at a time: mixing "run-on" notation with conventional notation is a no-no. 0.031 moles? Maybe. 18.4 l? No.

What's the "molecular mass" for hydrogen?

What do you mean by "run on" notation? and H=1.01g/mol
 
Make sure you take into account that hydrogen is a diatomic gas H2 so the molecular mass for hydrogen is 2.02 amu
 
htrrht said:
A piece of iron was added to a beaker that contained 0.585 mol/L copper(II) sulfate, CuSO4(aq). The solid copper that precipitated was dried, and its mass was found to be 5.02 g. Some unreacted iron remained in the beaker. Calculate the minimum volume of the copper(II) sulfate solution.

How many moles of copper were produced?

How many moles of copper sulfate were needed for that?

What volume of 0.585 M copper sulfate solution contains this number of moles?
 

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