W(s) + 3/2 O2 (g) = WO3 (s); delta H = -842.9 KJ
C (graphite) + O2 (g) = CO2 (g); delta H = -393.5 KJ
WO3 (s) + CO2 (g) = WC (s) + 5/2 O2 (g) delta H = +1195.5 kj
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W(s) + C(graphite) = WC (s) delta H = -40.9 kj
Hence delta H of the reaction is -40.9 kj c
Determine the ethalpy of reaction, delta H, for the formation of tungsten carbide, WC, from the...
rd enthalpy of formation for compound WC(s) from Wis) and Clgraphite) is difficult to measure directly because the reaction occurs at 1400°C w(s) + C(graphite) → WC(s) H combustion of the elements and of tungsten carbide can be measured and are given b However, the heats of 2w(s) + 302(g) → 2W03(s) C(graphite) + O2(g) → CO2(g) 2wc(s) + 502(g) → 2W03(s) + 2CO2(g) Δ H =-1680.6 kJ Δ H =-393.5 kJ Δ H =-2391.6 kJ Use Hess law and...
Tungsten carbide (WC) is an extremely hard material that is often used to create or coat cutting tools. Calculate the enthalpy of formation of solid tungsten carbide from tungsten metal and graphite given the following three pieces of information. Show your full working clearly (7 points) (i) AHr (WO3)-842.9 k/mol )AH (CO2)-393.5 kJ/mol (i) 2 WC (s)5O2 (g)2 WOs (s)+2 CO2 () AHn-2391.8 k 4.
Determine Heat of reaction (Hrxn) for: 2 C (s, graphite) + 3 H2 (g) ------> C2H6 (g) from the following C (s, graphite) + O2 (g) ------> CO2 (g) delta H = -393.5 kJ H2 (g) + 1/2 O2 (g) ------> H2O (l) delta H = -285.8 kJ 2 C2H6 (g) + 7 O2 (g) ------> 6 H2O (l) + 4 CO2 (g) delta H = -3,119.6 kJ
5. Use the following data to determine the delta H for the conversion of diamond into graphite: C(diamind) (s) + O2(g) = CO2(g) delta H degrees = -395.4 kJ 2CO2(g) = 2 CO(g) + O2(g) delta H degrees = 566.0 kJ 2CO(g) = C(graphite) (s) + CO2 (g) delta H degrees = -172.5 kJ C(diamond) (s) = C(graphite) delta H degrees = ?
From the following heats of combustion, CH3OH(l) + 3/2O2(g) → CO2(g) + 2H2O(l) ΔHorxn = –726.4 kJ/mol C(graphite) + O2(g) → CO2(g) ΔHorxn = –393.5 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔHorxn = –285.8 kJ/mol Calculate the enthalpy of formation of methanol (CH3OH) from its elements. C(graphite) + 2H2(g) + ½O2(g) → CH3OH(l) Methanol (CH3OH) is an organic solvent and is also used as a fuel in some automobile engines. From...
Use the example shown to calculate the reaction enthalpy, delta H, for the following reaction: CH4(g)+2O2(g)->CO2(g)2H2O(l). Use the series of reaction that follows: 1. C(s)+2H2(g)-> CH4(g), delta H= -74.8 kJ 2. C(s)+O2(g)->CO2(g), delta H= -393.5 kJ 3. 2H2(g)+O2(g)-> 2H2O(g), delta H= -484.0 kJ 4. H2O(l)->H2O(g), delta H= 44.0 kJ
1. Using the reactions given below please calculate the change in enthalpy (delta H) for the stated reaction. Stated Reaction: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) delta H = ?! Given Reactions & Enthalpy Changes: 2 Fe(s) + 3/2 02(g) → Fe2O3(s) 2 Fels) * delta H = -824.2 kJ delta H = -282.7 kJ CO(g) + 4 02(g) → CO2(g) 2. Using the reactions given below please calculate the change in enthalpy (delta H) for...
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation of one mole of substance from its constituent elements in their standard states. Thus, elements in their standard states have ΔH∘f=0. Heat of formation values can be used to calculate the enthalpy change of any reaction. Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) with heat of formation values given by the following table: Substance ΔH∘f (kJ/mol) NO(g) 90.2 O2(g) 0 NO2(g) 33.2 Then the standard heat...
a Using the heats of formation below, calculate the heat of reaction for the following reaction: C2H2(g) + 5/202(2)→ 2C02() +H20() AH® (kJ/mol) C2H2(g) 226.7 O2(g) 0 CO2(g) -393.5 H20(-285.8 kJ Submit b Using the heats of formation below. calculate the heat of reaction for the following reaction: PC13(2) + Cl2(2)→ PC15(e) AH(kJ/mol) PC13(g) -306.4 Cl2(E) 0 PC1s() -398.9
Use standard enthalpies of formation to determine Delta H degree_rxn for the reaction: Cr_2O_3(s) + 3CO(g) rightarrow 2 Cr(s) + 3CO_2(g) A) 69.7 kJ B0 -856.7 kJ C) 290.kJ D) -2651.7 kJ