Answer:
Step 1: Calculate the moles from mass
We know, moles = mass / molar mass
moles of C8H18 = 7 g / 114.23 g/mol = 0.06128 mol
Step 2: Calculation
(1) Write the equation
2 C8H18 + 25O2---> 16CO2 +18H2O ; ΔH=−11020 kJ
For 2 moles of C8H18 enthaply released = 11020 kJ
so, for 0.06128 mol of C8H18 enthapy released will be = ( 11020 kJ / 2 mol ) × 0.06128 mol = 338 kJ
Hence the enthalpy released = 338 kJ -----option(8) (last one)
Question 1 2C8H18 + 2502 - 16CO2 + 18H20 AH rxn--11020 kJ/mol rxn Look at above...
4) What is AH°rxn for the following reaction? 2C8H18(1) + 1702(g) → 16CO(g) + 18H20(1) Use the 2 reactions below: 2C8H18(1) + 2502(g) → 16CO2(g) + 18H20(1) 2CO(g) + O2(g) → 2C02(g) AH°rxn =-11020. kJ/mol AH°rxn =-566.0 kJ/mol A) -6492 kJ/mol B) +6492 kJ/mol C) -1964 kJ/mol D) -11020. kJ/mol E) -11586 kJ/mol
2C8H18 + 25O2 → 16CO2 + 18H2O ΔH° rxn = -11020 kJ/mol rxn Look at above equation. How many kJ of heat will be released when 7.00 grams of C8H18 is combusted? Which of the following would be endothermic ? 2Na + Cl2 ---> 2NaCl CH4 + 2O2 --> CO2 + 2H2O changing a solid iron nail to molten iron by melting it an iron nail rusts paper burns The sign of ∆H for the process NaCl( s) --> NaCl( l)...
For the following reaction: 2C3H18(1) + 2502(g) → 16C02(g) + 18H20(1) Compound AH°F (kJ moll) Sº (3 mol-1 K-1) C8H18 ( 259.30 328.00 O2 (g) 0.00 205.70 CO2 (9) -393.51 213.74 H20 (1) -285.83 69.91 Determine the temperature (to two decimal places in K) such that the reaction is in equilibrium in its standard states.