Given the following balanced thermochemical equation, predict the enthalpy chang

Question

Given the following balanced thermochemical equation, predict the enthalpy change if 2.0 mol of S8(s) reacts with excess H2(g).
S8 (s) + 8 H2 (g) 8 H2S (g) H = -160 kJ/mol
a. -320 kJ b. -160 kJ c. -80 kJ d. -180 kJ

Use the listed standard heats of formation to calculate the enthalpy change for the reaction below:
CO(g) + H2O(g) CO2(g) + H2(g)
Substance H°f
CO(g) -110.5 kJ/mol
CO2(g) -393.5 kJ/mol
H2(g) 0.0 kJ/mol
H2O(g) -241.8 kJ/mol
H2O(l) -285.8 kJ/mol
a. 261.7 kJ b. 568.8 kJ c. -41.2 kJ d. 789.8 kJ

Use the listed bond energies to estimate the enthalpy change for the reaction below:
CO(g) + H2O(g) CO2(g) + H2(g)
Bond Average Dissociation Energy
H—H 436 kJ/mol
O—H 460 kJ/mol
C=O 799 kJ/mol
C O 1070 kJ/mol
a. 295 kJ b. -44 kJ c. 755 kJ d. 828 kJ

Combine the two balanced thermochemical equations below in the appropriate manner, and use Hess’ Law to determine the unknown reaction enthalpy for the third reaction below.
MgO (s) + 2 HCl (aq) MgCl2 (aq) + H2O (l) Hrxn = -151 kJ
Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g) Hrxn = -467 kJ
Mg (s) + H2O (l) MgO (s) + H2 (g) Hrxn = ?
a. 316 kJ b. -316 kJ c. 618 kJ d. -618 kJ

Please show work

Explanation / Answer

a -320kJ/mol

c -41.2 kJ/mol

b -44kJ/mol

b -316kJ/mol

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