Answer:
should be appendix, I can't see any image tho.
The reaction for the formation of MgO(s):
2 Mg (s) + O2(g) -à
2MgO(s) ΔH = -601.24
kJ/mol
<span>The enthalpy
information is taken from: http://webbook.nist.gov/cgi/inchi?ID=C1309484&Mask=2</span>
From the equation and with an enthalpy change of -231 kJ:
-231 kJ * 2 mol Mg * (1/-601.24 kJ/mol) = 0.76841 mol Mg
Then, with the molar mass of MgO = 40.3,
0.76841 mol Mg *(2 mol MgO/2 mol Mg)* 40.3 g/mol MgO = <span>30.967 g MgO</span>
Answer:
6.45 joules
Explanation:
energy=10×(55-50)×0.129
=1.29×5
=6.45 J
hope this helps
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<span>Answer:
1/4 is the average bond order for a pâ’o bond (such as the one shown in blue) in a phosphate ion.</span>
