Hess's Law
Given the following data:
P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0
kJ
PH3(g) + 2O2(g) →
H3PO4(l) ΔH°= -1272.0 kJ
2P(s) + 5/2O2(g) → P2O5(s)
ΔH°= -1492.0 kJ
H2(g) + 1/2O2(g) → H2O(l) ΔH°=
-286.0 kJ
calculate ΔH° for the reaction:
H3PO4(l) → 1/2P2O5(s) +
3/2H2O(l)
ΔH°=??
also please explain how you found the answer
Hess's Law Given the following data: P(s) + 3/2H2(g) → PH3(g) ΔH°= +5.0 kJ PH3(g) +...
2. Given the following data: H2O(l) → H2(g) + 1/2O2(g) ΔH° = 285.8 kJ 2HNO3(l) → N2O5(g) + H2O(l) ΔH° = 76.6 kJ 2N2(g) + 5O2(g) → 2N2O5(g) ΔH° = 28.4 kJ Calculate ΔH° for the reaction: 1/2N2(g) + 3/2O2(g) + 1/2H2(g) → HNO3(l) Note that you should be able to answer this one without needing to use any additional information from the thermo table. I've attempted this question multiple times. I am able to get to the simplified eqaution...
Consider the following data. 2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ N2O5(g) + H2O(l) 2 HNO3(l) ΔH = -92.0 kJ N2(g) + 3 O2(g) + H2(g) 2 HNO3O(l) ΔH = -348.2 kJ Use Hess's law to calculate ΔH for the reaction below. 2 N2O5(g) 2 N2(g) + 5 O2(g) ΔH = _____kJ
12. Use Hess's Law to find AH for this reaction. (5) NO2(g) +2H2(g) ---> 2H2O(e) + NHs(g) Given the following two equations: 2NH3(g) -->N2(g) + 3H2(g) AHo +92 kJ 2N2(g)+ 2H2O(l) ---> NO2(g) + 2H2(g) AH° = +170 kJ
Given the following data: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ΔH = -2600 kJ C2H2(g) + 2H2(g) → C2H6(g) ΔH = -312 kJ 2H2(g) + O2(g) → 2H2O(l) ΔH = -572 kJ Find the ΔH of the following reaction: 4CO2(g) + 6H2O(l) → 2C2H6(g) + 7O2(g)
Hess's Law (b) Given the following thermochemical data: 2HNO3(aq) +A920(s) - H2O(1) +2AgNO3(aq) AH = -44.8 kJ Ag20(s) - 2Ag(s) + 1/2O2(9) AH = 31.0 kj H20(1) - H2(9)+1/202(9) AH = 285.8 kJ Use Hess's Law to determine AH for the reaction: Ag(s)+HNO3(aq) → 12H2(9)+AgNO3(aq) AH =
Using Hess's Law, calculate ΔH°R Equation: B2H6 (g) + 6 Cl2 (g) --> 2BCl3 (g) + 6 HCl (g) Given these 3 equations: (please show all work) BCl3 (g) + 3H2O (l) --> H3BO3 (g) + 3HCl (g) (ΔH°R = -112.5 KJ/mol BCl3) B2H6 (g) + 6H2O (l) --> 2H3BO3 (g) + 6H2 (g) (ΔH°R = -493.4 KJ/mol B2H6) H2 (g) + Cl2 (g) --> 2HCl (g) (ΔH°R = -184.6 KJ/mol H2)
For the following reaction: 2Na(s) + 2H2O(l) → 2NaOH(s) + H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) Na (s) 0.00 51.30 H2O (l) -285.83 69.91 NaOH (s) -425.93 64.46 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 391.96 K for this reaction. Assume ΔH°f and S° do not vary as a function of temperature.
a) Use Hess's law to calculate the enthalpy change for the reaction: 3C(s) + 4H2(g) + ½O2(g) → C3H8O(l) Given the following thermochemical equations: 2C3H8O(l) + 9O2(g) → 6CO2(g) + 8H2O(l) ΔH = -4042.6 kJ/mol C(s) + O2(g) → CO2(g) ΔH = -393.51 kJ/mol H2(g) + ½O2(g) → H2O(l) ΔH = -285.83 kJ/mol (in kJ/mol) A: -267.7 B: -302.6 C: -341.9 D: -386.3 E: -436.5 F: -493.3 G: -557.4 H: -629.9 b) Define if the following statement is an endothermic process or exothermic...
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
Use Hess's law and the following data CH4(g) + 2O2(g) → CO2(g) + 2 H2O(g) AH° = -802 kJ mol-1 CH4(8) + CO2(g) —> 2CO(g) + 2 H2(g) AFH° = +247 kJ mol-1 CH4(g) + H2O(g) –> CO(g) + 3H2(g) AFH° = +206 kJ mol-1 to determine A.Hº for the following reaction, an important source of hydrogen gas CH4(8) + +02(8) — CO(g) + 2 H2(8)