Consider the following reaction:
2Mg(s)+O2(g)→2MgO(s)ΔH=−1204kJ
a. How many grams of MgO are produced during an enthalpy change of -95.0 kJ ?
b. How many kilojoules of heat are absorbed when 7.60 g of MgO(s) is decomposed into Mg(s) and O2(g) at constant pressure?
We can write it as
2Mg(s)+O2(g)→2MgO(s) ΔH∘rxn=−1204⋅kJ⋅mol−1 (i)
To make the calculation easier we could write........
Mg(s)+12O2(g)→MgO(s) ΔH∘rxn=−602⋅kJ⋅mol−1 (ii)
And if −96.0⋅kJ energy are generated, with respect to MgO, this requires a molar quantity of −96.0⋅kJ/−602⋅kJ⋅mol−1=0.159⋅mol of rxn (ii), i.e. 0.159⋅mol×24.3⋅g⋅mol−1=3.88⋅g with respect to magnesium.
when 7.6⋅g MgO is decomposed to Mg and O2
7.6g/24.3⋅g⋅mol−1×−602⋅kJ⋅mol−1=−188.28⋅kJ
Hope you will get it
Consider the following reaction: 2Mg(s)+O2(g)→2MgO(s)ΔH=−1204kJ a. How many grams of MgO are produced during an enthalpy...
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