Based on the data below, determine the Delta H_f degree value for HCI gas. CH_4(

Question

Based on the data below, determine the Delta H_f degree value for HCI gas. CH_4(g) + Cl_2(p) rightarrow CCI_4(l) + HCI(g) [unbalanced] Delta H_rxn degree = -433 kJ Delta H_f degree (CH_4, g) = -74.87 kJ/mol Delta H_f degree (CCI_4, l) = -139 kJ/mol A. -92.31 kJ/mol B. -369 kJ/mol C. +124 kJ/mol D. Insufficient data to determine Use the thermochemical equations shown below to determine Delta H_rxn degree for: 3 H_2(g) + O_3(g) rightarrow 3 H_2O(g) [balanced] Eqn 1: 2H_2(g) + O_2(g) rightarrow 2 H_20(g) Delta H_1 degree = -483.6 kJ Eqn 2: 3 O_2(g) rightarrow 2 O_3(g) Dewlta H_2 degree = 284.6 kJ A. -199.0 kJ B. -583.1 kJ C. -867.7 kJ D. -1593.1 kJ

Explanation / Answer

24)
1st balance the equation

CH4 (g)+ 4Cl2 (g) ---> CCl4 (l) + 4HCl (g)

cCl2 is in elemental state
so, Hof (Cl2(g)) = 0 KJ/mol

Horxn = Hof (product) - Hof (reactant)
= Hof (CCl4(l)) +4* Hof (HCl(g)) - Hof (CH4(g)) - 4*Hof (Cl2(g))
-433 = -139 + 4*Hof (HCl(g)) - (-74.87) - 4*0
-433 = 4*Hof (HCl(g)) -64.13
Hof (HCl(g)) = -92.2 KJ/mol

Answer: A

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