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30 May 2020

The rusting of iron can be described by the following reaction:

If 1.00 mol of Fe(OH)3 (iron rust) is produced in a 3.00 L vessel from excess iron and water, what was the concentration of oxygen used?

 

Booster class
General Chemistry 2
Skill
Relate equilibrium concentrations of reactants and products
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Nestor Rutherford
Nestor RutherfordLv2
1 Sep 2020

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Related questions


Be sure to answer all parts.

Deterioration of buildings, bridges, and other structures through the rusting of iron costs millions of dollars every day. Although the actual process also requires water, a simplified equation (with rust shown as Fe2O3) is:
4 Fe(s) + 3 O2(g)

→

2 Fe2O3(s)

Δ

Hrxn = −1.65

×

103 kJ

(a) What is the ΔHrxn when 0.250 kg of iron rusts?

×

10 kJ

(b) How much rust forms when 6.80

×

103 kJ of heat is released?

×

10 g Fe2O3

The metathesis reaction between iron (111) nitrate and potassium hydroxide is shown below.
Fe(NO3)3(aq) +3KOH(aq) arrow 3KNO3(aq)+ Fe(OH)3(s)
How many grams of solid iron (111) hydroxide can be produced by the reaction of 400.0ml of 0.350M iron(111) nitrate solution with 225.0ml of 0.400M potassium hydroxide solution ?
determine the final concentration of each iron in solution at the end of the precipitation reaction

K,NO3,Fe,OH

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