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wariber [46]
3 years ago
7

If 8.00 g NH4NO3 is dissolved in 1000 g of water, the water decreases in temperature from 21.00 degrees Celsius to 20.39 degrees

Celsius. Determine the molar heat of solution of the ammonium nitrate.
Chemistry
1 answer:
telo118 [61]3 years ago
7 0

Answer:

25.7 kJ/mol

Explanation:

There are two heats involved.

heat of solution of NH₄NO₃ + heat from water = 0

q₁  +  q₂  =  0

n  =  moles of NH₄NO₃  =  8.00 g NH₄NO₃  ×  1 mol NH₄NO₃/80.0 g NH₄NO₃          

∴ n =   0.100 mol NH₄NO₃

q₁ = n * ΔHsoln = 0.100 mol * ΔHsoln

m  =  mass of solution  =  1000.0 g + 8.00 g  =  1008.0 g

q₂  =  mcΔT  = 58.0 g  ×  4.184 J°C⁻¹  g⁻¹  × ((20.39-21)°C) = -2570.19 J

q₁  +  q₂  =  0.100 mol  ×ΔHsoln  – 2570.19 J  =  0

ΔHsoln  =  +2570.19 J  /0.100 mol  =  +25702 J/mol  =  +25.7 kJ/mol

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1 year ago
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Answer:

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Explanation:

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1st step Ballance the equation. Afterwards, you can work properly

1 mol of Fe2O3 reacts with 3 moles of CO to make 2 moles of Fe and 3 moles of CO2

2nd step Predict the reactant in excess and limitant reagent.

If 1 moles of Fe2O3 reacts with 3 moles of CO

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I have 9 moles of CO, so the Fe2O3 is my limitant reagent.

<u><em>REMEMBER</em></u> you always have to work with the limitant.

If 3 moles of CO reacts with 1 mol of Fe2O3

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I have 2 moles of Fe2O3, so I still have Fe2O3, by the way the CO is the reactant in excess. (Just to show all)

3rd step Work with the limitant reagent.

1 mol of Fe2O3 ___ makes____ 2 moles of Fe  +  3 moles of CO

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