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lord [1]
2 years ago
13

The enthalpy change for the explosion of ammonium nitrate with fuel oil is –7198 kJ for every 3 moles of NH4NO3. What is the ent

halpy change for 1.0 mole of NH4NO3 in this reaction?
Chemistry
1 answer:
anastassius [24]2 years ago
7 0

Answer:

−2399.33 kJ

Explanation:

If NH₄NO₃ reacts with fuel oil to give a ΔH of -7198 for every 3 moles of NH₄NO₃

What is the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction

∴ For every 1 mole, we will have \frac{1}{3} of the total enthaply of the 3 moles

so, to determine the 1 mole; we have:

\frac{1}{3}*(-7198kJ)

= −2399.33 kJ

∴ the enthalpy change for 1.0 mole of NH₄NO₃ in this reaction = −2399.33 kJ

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Enter the chemical equation 2H+(aq)+S2−(aq)→H2S(g). Express your answer as a chemical equation.
amm1812

Answer : The complete chemical equation is,

2H^+(aq)+S^{2-}(aq)\rightarrow H_2S(aq)

Explanation :

As we know that, in a chemical equation the reacting species present on left side and the product formed present on right side and a right arrow inserted between the reactants and product that show a chemical reaction taking place.

In the chemical reaction, the phases of the substances are also included and subscripts and superscripts are also used for the numbers.

For the given chemical reaction, the balanced chemical equation including the phases, is given by:

2H^+(aq)+S^{2-}(aq)\rightarrow H_2S(aq)

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murzikaleks [220]

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