Ethane combusts completely, in accordance with this chemical pathway: 2C↓2H↓6(g) + 7O↓2(g) > 4CO↓2(g) + 6H↓2O(g), ΔH = ?
The enthalpies of the following elementary steps are known:
2C(s) + 3H↓2(g) > C2H↓6(g), ΔH = -84.7kJ/mol
C(s) + O↓2(g) > CO↓2(g), ΔH = -394kJ/mol
H2(g) + (1/2)O2(g) > H2O(g), ΔH = -242kJ/mol
Use the known enthalpies to determine the overall enthalpy of the process described in the balanced combustion equation above.

i know insulin is primary but i dont know the others im sorry

explanation:

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally

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