The enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) can be calculated using Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step in the reaction.

The first reaction is 2Fe(s)+O2(g)→2FeO(s) with ΔH = -544 kJ. We need to multiply this reaction by 2 to get 4Fe(s)+2O2(g)→4FeO(s) with ΔH = -1088 kJ.

The second reaction is 4Fe(s)+3O2(g)→2Fe2O3(s) with ΔH = -1648 kJ. This reaction is in the correct form for our desired reaction.

The desired reaction is 4FeO(s)+O2(g)→2Fe2O3(s). According to Hess's Law, the enthalpy change for this reaction is the sum of the enthalpy changes for the steps, which is -1088 kJ (from the first reaction) + -1648 kJ (from the second reaction) = -2736 kJ.

However, we need to consider that the first reaction is in the opposite direction of the desired reaction. Therefore, we need to change the sign of the enthalpy change for the first reaction. So, the enthalpy change for the desired reaction is 1088 kJ (from the first reaction) - 1648 kJ (from the second reaction) = -560 kJ.

So, the correct answer is not listed in the options A, B, C, or D. The correct enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) is -560 kJ.

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The enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) can be calculated using Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step in the reaction.

The first reaction is 2Fe(s)+O2(g)→2FeO(s) with ΔH = -544 kJ. We need to multiply this reaction by 2 to get 4Fe(s)+2O2(g)→4FeO(s) with ΔH = -1088 kJ.

The second reaction is 4Fe(s)+3O2(g)→2Fe2O3(s) with ΔH = -1648 kJ. This reaction is in the correct form for our desired reaction.

The desired reaction is 4FeO(s)+O2(g)→2Fe2O3(s). According to Hess's Law, the enthalpy change for this reaction is the sum of the enthalpy changes for the steps, which is -1088 kJ (from the first reaction) + -1648 kJ (from the second reaction) = -2736 kJ.

However, we need to consider that the first reaction is in the opposite direction of the desired reaction. Therefore, we need to change the sign of the enthalpy change for the first reaction. So, the enthalpy change for the desired reaction is 1088 kJ (from the first reaction) - 1648 kJ (from the second reaction) = -560 kJ.

So, the correct answer is not listed in the options A, B, C, or D. The correct enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) is -560 kJ.

Knowee AI · Accepted Answer

The enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) can be calculated using Hess's Law, which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step in the reaction.

The first reaction is 2Fe(s)+O2(g)→2FeO(s) with ΔH = -544 kJ. We need to multiply this reaction by 2 to get 4Fe(s)+2O2(g)→4FeO(s) with ΔH = -1088 kJ.

The second reaction is 4Fe(s)+3O2(g)→2Fe2O3(s) with ΔH = -1648 kJ. This reaction is in the correct form for our desired reaction.

The desired reaction is 4FeO(s)+O2(g)→2Fe2O3(s). According to Hess's Law, the enthalpy change for this reaction is the sum of the enthalpy changes for the steps, which is -1088 kJ (from the first reaction) + -1648 kJ (from the second reaction) = -2736 kJ.

However, we need to consider that the first reaction is in the opposite direction of the desired reaction. Therefore, we need to change the sign of the enthalpy change for the first reaction. So, the enthalpy change for the desired reaction is 1088 kJ (from the first reaction) - 1648 kJ (from the second reaction) = -560 kJ.

So, the correct answer is not listed in the options A, B, C, or D. The correct enthalpy change for the reaction 4FeO(s)+O2(g)→2Fe2O3(s) is -560 kJ.

Consider the two reactions involving iron and oxygen. 2Fe(s)+O2(g)→2FeO(s)Δ𝐻Θ=−544 kJ4Fe(s)+3O2(g)→2Fe2O3(s)Δ𝐻Θ=−1648 kJWhat is the enthalpy change, in kJ, for the reaction below?4FeO(s)+O2(g)→2Fe2O3(s)A. −1648−2(−544)B. −544−(−1648)C. −1648−544D.

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