ZnC4H10 is liquid that spontaneously undergoes combustion in the presence of air according to the following equation
ZnC4H10 (l) + O2 (g) ---> ZnO (s) + CO2 (g) + H2O (g)
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ZnC4H10 is liquid that spontaneously undergoes combustion in the presence of air according to the following...
ZnC4H10 is liquid that spontaneously undergoes combustion in the presence of air according to the following equation ZnO (s) + CO2 (g) ZnC4H10 (1) + O2 (g) + H2O (g) 1. Balance the equation. 2. Calculate w and AE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The AH vaporization is 39.9 kJ/mol at 265 K.
Calculate w and ΔE when 2 mol of liquid ZnC4H10 is vaporized at 265 K and 760 mm Hg. The ΔH vaporization is 39.9 kJ/mol at 265 K.
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
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pt) A sample of 1.0 mol of liquid octane C8H18(1) undergoes combustion accord 5. (10 pt) A C3H18(0) + O2(g) → 8 CO2(g) + 9 H2O(l) Using the standard enthalpies of formation given calculate the change in enthalpy in kJ/mol associated with the combustion of 1.0 mol of C8H18(1) at 1.0 bar pressure and 25 °C. Substance AH® (kJ/mol) C8H18() -249.9 CO2(g) -393.51 H2O) -285.83
Question 3 Propane (C3Hg) undergoes combustion according to the following thermochemical equation: C3H8(g) + 5 O2(g) - 3 CO2(g) + 4H2O(g) AHrxn=-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 C3Hg a. -104.7 kJ/mol O b. +1407.7 kJ/mol O C. -1407.7 kJ/mol O d. +104.7 kJ/mol o e. -4190.7 kJ/mol uestion 4 Consider the evaporation of liquid water to water vapor at 125°C. What is true...
Combustion of 2.14 g of liquid benzene (C 6H 6) causes a temperature rise of 16.2 °C in a constant-pressure calorimeter that has a heat capacity of 5.53 kJ/°C. What is Δ H for the following reaction? C6H6(l) + O2(g) → 6 CO2(g) + 3 H2O() a. 89.5 kJ/mol-rxn b. –3.27 × 103 kJ/mol-rxn c. –41.8 kJ/mol-rxn d. –89.5 kJ/mol-rxn e. 41.8 kJ/mol-rxn
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
(a) For the combustion of 0.05146 mol of C5H12O (l) at constant pressure and a temperature of 25.00oC, 171.2 kJ of heat liberated by this reaction is measured. With this data, what are the values of ΔH, ΔU, Q, and W for the combustion of 1,000 moles of C5H12O (l) at constant volume and a temperature of 25.00oC? Combustion is the reaction of a substance with O2 (g) to produce CO2 (g) and H2O (l). (b) We have an unknown...
Determine the heat involved in the combustion of liquid hydrazine by using the following reactions. Use the balanced equation determined on the previous slide to begin. 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(ℓ) ΔH° = –1013 kJ/mol N2O(g) + 3H2(g) → N2H4(ℓ) + H2O(ℓ) ΔH° = –317 kJ/mol 2NH3(g) + ½O2(g) → N2H4(ℓ) + H2O(ℓ) ΔH° = –142.9 kJ/mol H2(g) + ½ O2(g) → H2O(ℓ) ΔH° = –285.8 kJ/mol Launching a small spacecraft to study Jupiter required approximately 28 million...
The combustion of lauric acid is given by the following
thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) +
12 CO2(g) Hcomb is −7377 kJ mol−1 Using the heats of formation
for CO2(g) and H2O(l) calculate the heat of formation (△fH) of
lauric acid. △fH△ CO2(g) = −393.5 kJ mol−1 fH
H2O(l)= −285.8 kJ mol−1
19. The combustion of lauric acid is given by the following thermochemcial equation: CH3(CH2)10COOH(s) + 18 O2(g) → 12 H2O(l) + 12 CO2(g) AH...