Using Hess's Law to calculate net reaction enthalpyStella vNitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step,nitrogen and hydrogen react to form ammonia:N,(g) + 3 H,(g) - 2 NH,(g)AH=-92. kJIn the second step, ammonia and oxygen react to form nitric acid and water:NH,(g) + 20,(g) → HNO,(g) + H,O(g)AH =-330. kJdoCalculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions.Round your answer to the nearest kJ.團ExplanationCheckO 2020 McGraw-Hill Education. All Rights Reserved Taorms of Use Privacy Accessibilty414 PM10/31/2020O Type here to searchhpthefraf128endprt scdeletehome14440numlockbackspace%24%3D%2356.7.8.6.

The first chemical equation is, N2g+3H2g→2NH3g ∆H=-92 kJ......(1) The second chemical equation is, NH3g+2O2g→HNO3g+H2Og ∆H=-330 kJ......(2)Multiply equation (2) by 2. 2NH3g+2O2g→HNO3g+H2Og ∆H=-330 kJ2NH3g+4O2g→2HNO3g+2H2Og ∆H=-660 kJ......(3) Add equation (1) and equation (3). N2g+2NH3g+3H2g+4O2g→2NH3g+2HNO3g+2H2Og ∆H=-92 kJ+-660 kJ The final equation is expressed as, N2g+3H2g+4O2g→2HNO3g+2H2Og ∆H=-752 kJ......(4) The above reaction shows that the enthalpy of reaction for the formation of two moles of nitric acid is -752 kJ.Divide equation (4) by 2. 12N2g+3H2g+4O2g→2HNO3g+2H2Og ∆H=-752 kJ12N2g+32H2g+2O2g→HNO3g+H2Og ∆H=-376 kJ The above reaction shows the net change in enthalpy for the formation of one mole of nitric acid is -376 kJ.Answer: The net change in enthalpy for the formation of one mole of nitric acid is -376 kJ.

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Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) + 3 H,(9) - 2 NH,(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g) + 20,(g) - HNO,(g) + H,O(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.

Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) + 3 H,(9) - 2 NH,(g) AH=-92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH,(g) + 20,(g) - HNO,(g) + H,O(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ.

Chemistry

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Using Hess's Law to calculate net reaction enthalpy
Stella v
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step,
nitrogen and hydrogen react to form ammonia:
N,(g) + 3 H,(g) - 2 NH,(g)
AH=-92. kJ
In the second step, ammonia and oxygen react to form nitric acid and water:
NH,(g) + 20,(g) → HNO,(g) + H,O(g)
AH =-330. kJ
do
Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions.
Round your answer to the nearest kJ.
團
Explanation
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2