Pentaborane BgHg(s) burns vigorously in 02 to give B203(s) and H201). Calculate AHrxn for the combustion of 5.00 mol of B5H9. AH{B2031s)) = -1,273.5 kJimol AH{B5H9/S)] = 73.2 kJimol AH(H200) = -285.8 kJ/mol Muitiple Choice - 22,700 kJ - 45,400 kJ 45,400 kJ - 9,090 kJ - 8,790 kJ
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- Calculate the enthalpy change when 1.0(1 g of methane is burned in excess oxygen according to the reaction CH,(g) 4- 2O2(g) ->CO2(g) + H-CH/) 1H = -891 kJ/molWhat is the enthalpy of reaction (in kJ/mol rxn) for CACO3{5) → CaO(s) + CO2(g) if Ca(s) + Cgraphite + 3/2 O21g) → CaCO3(s) with AH;= -1207 kJ/mol Ca(s) + 1/2 O2(g) CaO(s) with AH;= -635.5 kJ/mol Cgraphite + O2(g) → CO2{g) with AH;= -393.5 kJ/molPentaborane B5H9(s) burns vigorously in 02 to give B203(s) and H20(). Calculate AHpxn AH(B203(s)]=-1.273.5 kJ/mol AH{B5H9(s)] = 73.2 kJ/mol AH{H20()) = -285.8 kJ/mol for the combustion of 5.00 mol of BgHg. Multiple Choice 9,090 kJ - 22,700 kJ 1. 45,400 kJ - 8,790 kJ -45,400 kJ Next> LEGO
- CH,(9) + 2 O,(g) AH = -809.0 kJ/mol rxn Co,(9) + 2 H,0(g) ΔΗ. = -81.3 kJ 'cond 2 H,0U) Given the energy diagram above, what is AH when two moles of methane are combusted? -401.15 kJ +1604.6 kJ -802.3 kJ +802.3 kJ +401.15 kJ O -1604.6 kJCH,(g) + 2 0,(g) AH = -809.0 kJ/mol rxn co,(g) + 2 H,0(g) AH cond = -81.3 kJ 2 H,0(1) Given the energy diagram above, what is AH when 0.5 mol of methane is combusted? -802.3 kJ +802.3 kJ -1604.6 kJ +401.15 kJ +1604.6 kJ -401.15 kJCalculate the enthalpy change for the reaction below. Compound Нeat Value -> 3NO(s) ,0,ls) AH +174 k (belONH2 -(aloH (2Fo+ ('N AH -183 k AH =-128 k) 2NO(g) O-137 kJ O-128 kJ -174kJ 270KJ
- 2. Given the following heat of formation values, Calculate the heat of reaction for C;He) + Ozo) CO2(9) + H2O0 H; values in kJ/mol for: C;Ho) = -103.8 8(g) O2(9) = 0 CO20) -393.5 H,O = -285.8 a. 3.613 X 10² kJ b. -5.755 X 10?kJ с. 1. 413 X 10? kJ[References] Calculate AH for the reaction: 2NH3 (g) + O2(g) → N2H4 (1) + H2O(1) given the following data: 2NH3 (g) + 3N2O(g) → 4N2(g) + 3H2O(1) AH =–1010. kJ N2O(9) + ЗH2(9) — N;Ha (1) + Hа0(1) ДН %3D — 317 kJ N2H4 (1) + O2 (9) → N2(g)+2H20(1) ΔΗ--623 k.J На (9) + О2(9) — Н,0(1) AH = -286 kJ ΔΗ- kJ Submit Answer Try Another Version 3 item attempts remaining[Review Topics] [References] One cubic meter of methane hydrate has 164 m of CH, (at STP). If you burn the methane in 8.50 m of hydrate [to give CO2 (g) and H20(g)], how much energy, as heat, can be obtained? Species AƒH, kJ/mol CH4 (g) -74.87 02(g) 0. CO2(g) -393.509 H2O(g) -241.83 Energy obtained kJ %3D Submit Answer Retry Entire Group 4 more group aftempts remaining 10:11 PM FLU 3/21/2020
- 2. An experiment was carried out to determine the enthalpy change of combustion of propan-1-ol. The experimental set-up was shown below. a beaker water (500.0 cm³) propan-1-ol (a) Write the equation for the complete combustion of propan-1-ol (C;H¬OH). (b) Give a suggestion to the above set-up so as to minimize heat loss to the surroundings. (c) Burning 2.88 g of propan-1-ol caused the temperature of 500.0 cm³ of water to rise by 46.0°C. Calculate the enthalpy change of combustion of propan-1-ol. (Assume that the specific heat capacity and the density of water are 4.2 J g- K-l and 1.0 g cm- respectively.) (Molar mass of propan-1-ol: 60 g) -3 (d) The enthalpy change obtained in (c) cannot be called as 'standard enthalpy change'. Explain why.A.) What is the heat of reaction, ΔH°? CO2(g) + H2O(l) à H2CO3(aq) –20.2 kJ mol–1 –1379 kJ mol–1 –592 kJ mol–1 B.) What is the average bond energy in CO2? CO2(g) ΔH°f, = –393.5 kJ mol–1 CO(g) ΔH°f, = –110.5 kJ mol–1 C(g) ΔH°f, = +715 kJ mol–1 CO32–(aq) ΔH°f, = –676.3 kJ mol–1 O(g) ΔH°f, = +249.0 kJ mol–1 207 kJ mol–1 1607 kJ mol–1 804 kJ mol–1benzene, C6H6, gives thecompound special stability.(a) By using data in Appendix C, compare the heat of combustionof 1.0 mol C6H6(g) to the heat of combustion of 3.0 mol acetylene,C2H2(g). Which has the greater fuel value, 1.0 mol C6H6(g) or 3.0mol C2H2(g)? Are your calculations consistent with benzene beingespecially stable?