At room temperature the reaction of iron(III) oxide with carbon to produce solid

Question

At room temperature the reaction of iron(III) oxide with carbon to produce solid metallic iron and carbon monoxide has an equilibrium constant (K) on the order of 10^-58 and a positive delta S degree. 2Fe_2O_3(s) + 3C(s) rightarrow 4Fe(s) + 3CO_2(g) Despite its very low K at room temperature this reaction is widely used in industry to convert iron oxide into iron metal at very high temperatures. In fact, more than 100000000 tons of iron is made this way annually. Based on this information, what can we infer about this reaction at very high temperatures? The value of delta H degree must be negative and K increases with increasing temperature. The value of delta H degree must be negative and K decreases with increasing temperature. The value of delta H degree must be positive and K increases with increasing temperature. The value of delta H degree must be positive and K decreases with increasing temperature. Styrene (C_8H_8) IS a chemical used in the production of synthetic rubber. When styrene burns in oxygen to form carbon dioxide and liquid water under standard-state conditions at 25 degree C, 42.62 kJ are released per 1 gram of styrene. What is the standard enthalpy of formation of styrene at 25 degree. -637 kJ/mol -4432 kJ/mol +141 kJ/mol +324 kJ/mol

Explanation / Answer

30) The conversion of Fe2O3 to Fe by reaction with C, has a very low K value. The reaction is still employed at high temperature as,

A) The value of dHo muxt be negative and K increases with increasing temperature.

31) The combustion reaction,

C8H8 + 10O2 --> 8CO2 + 4H2O

42.62 = (8 x -393.5 + 4 x -286) - dHo[C8H8]

dHo[C8H8] = -4432 kJ/mol

B. -4432 kJ/mol

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.