Use the following thermochemical equations to calculate the standard enthalpy of formation of Mg(NO3)2(s). A,H° - - 3884 kJ mol- A,Hô - +463 k) mol-1 8Mg(s) + Mg(NO3)2(s) → M93N2(s) + 6M9O(s) M93N2(s) → 3Mg(s) + N¿(9) 2MgO(s) → 2Mg(s) + 02(g) A,Hô = +1203 kJ mol-1 M93N2(s) + 6M9O(s) → 8Mg(s) + Mg(NO3)2(s) kJ 3Mg(s) + N2(9) → M93N2(s) 4,48 = 6Mg(s) + 302(g) → 6M9O(s) Mg(s) + N2(g) + 302(g) → Mg(NO3)2(s)
Use the following thermochemical equations to calculate the standard enthalpy of formation of Mg(NO3)2(s). A,H° - - 3884 kJ mol- A,Hô - +463 k) mol-1 8Mg(s) + Mg(NO3)2(s) → M93N2(s) + 6M9O(s) M93N2(s) → 3Mg(s) + N¿(9) 2MgO(s) → 2Mg(s) + 02(g) A,Hô = +1203 kJ mol-1 M93N2(s) + 6M9O(s) → 8Mg(s) + Mg(NO3)2(s) kJ 3Mg(s) + N2(9) → M93N2(s) 4,48 = 6Mg(s) + 302(g) → 6M9O(s) Mg(s) + N2(g) + 302(g) → Mg(NO3)2(s)
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![Use the following thermochemical equations to calculate the standard enthalpy of formation of Mg(NO3)2(s).
8Mg(s) + Mg(NO3)2(s) → Mg,N2(s) + 6M9O(s)
A,H0 = - 3884 kJ mol-1
Mg;N2(s) → 3Mg(s) + N2(g)
4,48
+463 kJ mol-1
2M9O(s) → 2Mg(s) + 02(g)
4,48
= +1203 k) mol-1
M93N2(s) + 6Mgo(s) → 8Mg(s) + Mg(NO3)2(s)
kJ
3Mg(s) + N2(g) → Mg;N2(s)
kJ
6Mg(s) + 302(9)
+ 6M9O(s)
kJ
Mg(s) + N2(g) + 302(g) → Mg(NO3)2(s)
kJ](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6b484c6-e3f6-4297-ae09-03b7e68d48db%2F24404adc-b23d-4bcd-96c1-0dc2aae935ca%2Fe8ndks6_processed.png&w=3840&q=75)
Transcribed Image Text:Use the following thermochemical equations to calculate the standard enthalpy of formation of Mg(NO3)2(s).
8Mg(s) + Mg(NO3)2(s) → Mg,N2(s) + 6M9O(s)
A,H0 = - 3884 kJ mol-1
Mg;N2(s) → 3Mg(s) + N2(g)
4,48
+463 kJ mol-1
2M9O(s) → 2Mg(s) + 02(g)
4,48
= +1203 k) mol-1
M93N2(s) + 6Mgo(s) → 8Mg(s) + Mg(NO3)2(s)
kJ
3Mg(s) + N2(g) → Mg;N2(s)
kJ
6Mg(s) + 302(9)
+ 6M9O(s)
kJ
Mg(s) + N2(g) + 302(g) → Mg(NO3)2(s)
kJ
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