AP/IB Chemistry: Hess’s Law Problems WS#4 1. Calculate the value of Ho/kJ for the following reaction using the listed t

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AP/IB Chemistry: Hess’s Law Problems
WS#4
1. Calculate the value of Ho/kJ for the
following reaction using the listed thermochemical
equations:
P4O10(g) + 6 PCl5(g) 10
Cl3PO(g)
1/4 P4(s) + 3/2 Cl2(g) PCl3(g) Ho/kJ =
-306.4
P4(s) + 5 O2(g) P4O10(g) Ho/kJ = -2967.3
PCl3(g) + Cl2(g) PCl5(g) Ho/kJ =
-84.2
PCl3(g) + 1/2 O2(g) Cl3PO(g) Ho/kJ =
-285.7
2. Given the following equations and Ho values, determine
the heat of reaction (kJ) at 298 K for the
reaction:
2 SO2(g) + 2 P(s) + 5 Cl2(g) 2 SOCl2(l) + 2
POCl3(l)
SOCl2(l) + H2O(l) SO2(g) + 2 HCl(g)
Ho/kJ = +10.3 PCl3(l)
+ 1/2 O2(g) POCl3(l) Ho/kJ =
-325.7 P(s) + 3/2 Cl2(g) PCl3(l) Ho/kJ = -306.7 4 HCl(g) + O2(g) 2
Cl2(g) + 2 H2O(l) Ho/kJ = -202.6
3. Calculate the heat of combustion (kJ) of propane,
C3H8 using the listed standard enthapy of reaction
data:
C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(g)
3 C(s) + 4 H2(g) C3H8(g) Ho/kJ =
-103.8
C(s) + O2(g) CO2(g) Ho/kJ = -393.5
H2(g) + 1/2 O2(g) H2O(g) Ho/kJ = -241.8
4. Given the following equations and Ho values given
below, determine the heat of reaction at 298 K for the
reaction:
2 N2(g) + 5 O2(g) 2 N2O5(g)
2 H2(g) + O2(g) 2 H2O(l) Ho/kJ = -571.6 N2O5(g) + H2O(l)
2 HNO3(l) Ho/kJ = -73.7 N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) Ho/kJ =
-348.2
5. Given the following equations and Ho values,
determine the heat of reaction at 298 K for the
reaction:
C(s) + 2 H2(g) CH4(g)
C(s) + O2(g) CO2(g) Ho/kJ = -393.5 H2(g) + 1/2 O2(g)
H2O(l) Ho/kJ = -285.8 CO2(g) + 2 H2O(l) CH4(g) + 2 O2(g) Ho/kJ =
+890.3
6. Given the following equations and Ho values,
determine the heat of reaction (kJ) at 298 K for the
reaction:
B2H6(g) + 6 Cl2(g) 2 BCl3(g) + 6
HCl(g)
BCl3(g) + 3 H2O(l) H3BO3(g) + 3 HCl(g) Ho/kJ = -112.5
B2H6(g) + 6 H2O(l) 2 H3BO3(s) + 6 H2(g) Ho/kJ = -493.4 1/2 H2(g) +
1/2 Cl2(g) HCl(g) Ho/kJ = -92.3
7. Given the following equations and Ho values,
determine the heat of reaction (kJ) at 298 K for the
reaction:
2 OF2(g) + 2 S(s) SO2(g) + SF4(g)
OF2(g) + H2O(l) O2(g) + 2 HF(g) Ho/kJ = -276.6 SF4(g) +
2 H2O(l) 4 HF(g) + SO2(g) Ho/kJ = -827.5 S(s) + O2(g) SO2(g) Ho/kJ
= -296.9
8. Determine Ho/kJ for the following reaction using the
listed enthalpies of reaction:
N2H4(l) + 2 H2O2(g) N2(g) + 4 H2O(l)
N2H4(l) + O2(g) N2(g) + 2 H2O(l) Ho/kJ = -622.3 kJ H2(g)
+ 1/2 O2(g) H2O(l) Ho/kJ = -285.8 kJ H2(g) + O2(g) H2O2(l) Ho/kJ =
-187.8 kJ