2SO2 + O2= 2SO3 ΔH= -198KJ/MOLE
Here 2 moles of SO2 (M.Wt=2x32+32=96gr) on combustion produces 198 KJ of energy
320gr of SO2 produces is
320grx198/96gr= 6.6x102 KJ/mole
THE AMOUNT OF HEAT PRODUCED IN THE ABOVE REACTION IS 6.6X102 KJ/MOLE
How much heat is evolved if 0.600 kg of SO2 is burned in excess oxygen? 2SO2(g) + O2(g) → 2803(g) AH°rxn=-198 kJ/mol O 3.71x 103 kJ O 5.46 x 10-2k) 0 1.85 x 103 kg O 927 kJ O 59,400 kJ
please show me how to get the correct answers in preperation
for my upcoming exam
14.) A 15.) B
14. Given: 2 Al(s) + 3/2 O2(g) - Al2O3(s) Hºe - -1670 kJ for Al2O3(s) What is AH for the following reaction? 2 A1,0, (s) - 4 Al(s) + 3 O2(g) Hºrn - ? A. 3340 kJ B. 1670 kJ C. -3340 kJ D. -1670 kJ E . -835 kJ 15. Given the following thermochemical equation: 2 SO2(g) + O2(g) -...
Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for SO3(g): 2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -198 kJ ΔH°f (kJ/mol) SO2(g) -297
Please help with these two questions :(
1. How much energy (in kJ) is evolved during the reaction of
76.9 g of Al, according to the reaction below?
Fe2O3(s) + 2 Al(s) →
Al2O3(s) + 2 Fe(s) ΔH°rxn = -852
kJ
Assume that there is excess Fe2O3.
2. A 12.43 g sample of ethanol (C2H5OH) is
burned in a bomb calorimeter with a heat capacity, C = 5.65
kJ/°C.
C2H5OH(l) + 3 O2(g) → 2
CO2(g) + 3 H2O(g) ΔH°rxn...
The thermochemical equation for the combustion of sulfur dioxide is shown below. 2 S02(g) + O2 (g) + 2 So3(g) deltaH =-198 kJ What is the enthalpy change for the following reaction? 4 SO3(g) → 4 SO2(g) + 2 O2(g)
Use the AHⓇ and AH°rxn information provided to calculate AHºf for SO3(g): AHºf (kJ/mol) | 2 SO2(g) + O2(g) → 2 SO3(9) AH°rxn = -198 kJ SO2(g) -297 de parte a 2 500) • 03 * 2 500) 0 -578 kJ/mol 0 -248 kJ/mol 0 -495 kJ/mol 0 -396 kJ/mol 0 -792 kJ/mol Submit Request Answer Provide Feedback
Heat Evolved During Combustion Consider the following reaction: 2 CO(g) + O2(g) 2 CO2(9) Use standard heats of formation from Zumdahl 'Chemical Principles' 8th ed. Appendix Four pp A19 - A21. How much heat is evolved when 1.071x101 moles of CO(9) is burned in excess oxygen. Answer to 4 sig figs. 1pts Submit Answer Tries 0/5 How much heat is evolved when 1.681x102 g of CO(g) is burned in excess oxygen. Answer to 4 sig figs. 1pts Submit Answer Tries...
Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction: 4 SO3(g) → 4 S(s) + 6O2(g) ΔH°rxn = ? Given: SO2(g) → S(s) +O2(E) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g) → 2SO3(g) ΔH°rxn = -197.8 kJ-494.6 kJ -692.4 kJ -791.4 kJ 1583 kJ 293.0 kJ
Calculate heat for the following reaction to produce sulfur dioxide, S(3) + O2(g) = SO2(E) given the thermochemical equations below. 2 S(s) + 3 O2(g) =2 SO3(g) AH° = -791.5 kJ 2 SO2(g) + O2(g) = 2 SO3(g) AH° = -197 9 kJ Show all work and calculate to the correct number of sig figs.
Heat Evolved During Combustion and Heat Capacity of a
Gas at Constant Pressure
A.
Consider the following reaction:
2 C2H2(g) + 5
O2(g)
4 CO2(g) + 2H2O(l)
Use standard heats of formation from Zumdahl 'Chemical
Principles' 8th ed. Appendix Four pp A19 - A21.
a) How much heat is evolved when
1.440×101 moles of
C2H2(g) is burned in excess oxygen.
Answer to 4 sig figs.
b) How much heat is evolved when
2.250×102 g of CO2(g) is produced
from the...