Worksheets7.3 Thermochemical Equations
Total questions: 10
Worksheet time: 3hrs 30mins
Calculate ΔH when 2 moles of ethanol (C2H5OH) reacts with excess oxygen according to the following thermochemical equation?
C2H5OH + 3O2 → 2CO2 + 3H2O ΔH = −1366.7 kJ
-2733.4 kJ
-683.35 kJ
-1366.7 kJ
-910.67 kJ
What will ΔH be if there is 1 mole of oxygen?
4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1500 kJ
-500 kJ
500 kJ
-750 kJ
-4500 kJ
What is ΔH if 2 mol of O2(g) is reacted in this reaction?
H2(g) + ½ O2(g) → H2O(l) ∆H = -285.8 kJ
-570 kJ
-71.45 kJ
-1143.2 kJ
-142.9 kJ
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
C+ O2 --> CO2 + 60kJ, what heat is released for the reaction if 3 moles of CO2 is formed?
60 kJ
120 kJ
180 kJ
20 kJ
A negative ΔH means the reaction is:
complete
at equilibrium
exothermic
endothermic
A positive ΔH means the reaction is:
complete
at equilibrium
exothermic
endothermic
If ΔT is positive then heat is being ___________by the reaction, and if ΔT is negative then heat is being _____________by the reaction.
absorbed, released
released, absorbed
heat is staying the same
There is no way to know what is going on with the heat.
A hot iron ball having a mass 0.2 g and at
655°C is mixed with 5.0 g of water at 10°C . If the specific heat capacity of iron is 0.449 J/gC, what is the final temperature of the mixture? Assume the specific heat of the water is 4.184 J/gC
13°C
28°C
55°C
81°C
