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Page 2 of 7 Chem 1 Exercise # 3 Calculate the ΔΗ0n for the combustion of...
Using Hess's Law, calculate ΔH°R Equation: B2H6 (g) + 6 Cl2 (g) --> 2BCl3 (g) + 6 HCl (g) Given these 3 equations: (please show all work) BCl3 (g) + 3H2O (l) --> H3BO3 (g) + 3HCl (g) (ΔH°R = -112.5 KJ/mol BCl3) B2H6 (g) + 6H2O (l) --> 2H3BO3 (g) + 6H2 (g) (ΔH°R = -493.4 KJ/mol B2H6) H2 (g) + Cl2 (g) --> 2HCl (g) (ΔH°R = -184.6 KJ/mol H2)
Using the following equation for the combustion of propane, calculate the amount of propane consumed if the reaction gave off 333 kJ heat. C3H8(g) + 5 O2(g) --> 3 CO2(g) + 4 H2O(g) ΔH = -2044 kJ
calculate Δh0 ulate AHo (in kJ/mol) for the reaction: B2H6(g)+6 Cl2(g)2 BCls(g)+6 HCl(g) ven the following data: BCI5(g)+3 H2O(I) H3BO:(g)+3 HCl(g) AH° = -112.5 kJ/mol B2H&(g) + 6 H2O(1) 2 H3BO:(g) + 6 H2(g)AH°= -493.4 kJ/mol AHOC(HCI, g) -92.3 kJ/mol
1. Calculate the enthalpy of combustion (in kJ/mol) for propane, which burns according to the following equation: C3H8(g) + 5 O2(g) + 3 CO2(g) + 4H2O(1) AH® (C3H8) = -104.63 kJ/mol
Question 3 Propane (C3H8) undergoes combustion according to the following thermochemical equation: C3H8(g) + 5 O2(g) -- 3 CO2(g) + 4H2O(g) Arxn = -2043.0 kJ Substance Heat of Formation (kJ/mol) CO2(g) -393.5 H2O(g) -241.8 O2(g) 0 C3H8(g) ? Calculate the standard enthalpy of formation of propane C3H8 a. -104.7 kJ/mol ob. +1407.7 kJ/mol C. -1407.7 kJ/mol O d. +104.7 kJ/mol o e. -4190.7 kJ/mol
Energy 4. (3 points) How much heat is released when 150.0 g of copper cool down from 70.1°C to 22.3"C7 Specific hest capacity of copper is 0.385 g"C. 5. (3 points) During combustion of acetylene, CHą, according to the reaction below 1299 kJ are released: C Hz + 5/20, 200, + H2O AH = -1299 kJ How much energy is liberated when 100.0 of acetylene combust? 6.3 points) Given the following equations and AH values, determine the heat of reaction...
Given the enthalpies of combustion of propane (C3Hg), carbon and hydrogen, C3H3(g) + 5 O2(g) + 3 CO2(g) + 4 H20(1) AH° = -2219.9 kJ C(s) + O2(g) + CO2(8) AH° = -393.5 kJ 2 H2(g) + O2 + 2 H2O(1) AH° = -571.6 kJ Calculate the enthalpy of formation of propane. The reaction is shown below. 3 C(s) + 4H2(g) → C3H3(g)
Use the following information to calculate the heat of formation of propane C3H8. 3 C (S-Graphite) + 4 H2 (g) —› C3H8 (g) 1. C (S-Graphite) + O2 (g) —› CO2 (g) ΔH = - 393.5 kJ 2. H2 (g) + ½ O2 (g) —› H2O (l) ΔH = - 285.8 kJ 3. C3H4 (g) + 4 O2 (g) —› 3 CO2 (g) + 2 H2O (l) ΔH = - 1937 kJ 4. C3H6 (g) + 9/2 O2 (g) —›...
Calculate the volume change (in Liters) during the combustion of propane in which ΔE = -3083.67 kJ and ΔH = -3087.12 kJ at a constant pressure of exactly one atm and constant temperature. C3H8(g) + 5 O2(g) ↔ 3 CO2(g) + 4 H2O(l) The product of pressure and volume change should give units of L*atm. It can be shown that 1 L*atm = 101 J.
1.f) Methane gas (CH4) enters a combustion chamber at a rate of 3 kg/sec at a temperature of 25 °C. A 200% theoretical air is supplied at a temperature of 400K. At the middle of methane combustion process (i.e., after 50% of methane gas is burnt), liquid propane (C3H8) at 25°C is injected at a rate that produces neither CO nor O2 in the flue gases. Assume steady state and adiabatic process at 1 atm, calculate the following i. The...