Calculate the enthalpy of the reaction
4B(s)+3O2(g)→2B2O3(s)
given the following pertinent information:
B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ
2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ
H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ
H2O(l)→H2O(g), ΔH∘D=+44 kJ
Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(...
Part A Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ 12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ Express your answer with the appropriate units. Part B Calculate the enthalpy of the reaction 4B(s)+3O2(g)→2B2O3(s) given the following pertinent information: B2O3(s)+3H2O(g)→3O2(g)+B2H6(g), ΔH∘A=+2035 kJ 2B(s)+3H2(g)→B2H6(g), ΔH∘B=+36 kJ H2(g)+12O2(g)→H2O(l), ΔH∘C=−285 kJ H2O(l)→H2O(g), ΔH∘D=+44 kJ Express your answer with the appropriate units.
(a) Diborane (B2H6) is a highly reactive borohydride that can be used as rocket fuel. Calculate Δ? for synthesis from the elements as: 2B (s) + 3H2 (g) → B2H6 (g) Use the following data: 4B (s) + 3O2 (g) → 2B2O. (S) Δ? = -2546 kJ mol-1 B2H6 (g) + 3O2 (g) → B2O3 (s) + 3H2O (g) Δ? = -2035 kJ mol-1 2H2 (g) + O2 (g) → 2H2O (l) Δ? = -572 kJ mol-1 H2O (l) →...
Calculate the enthalpy of the reaction 2NO(g) + O2(g)2NO2(g) Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." It is important to recall the following rules: given the following reactions and enthalpies of formation: 1. ¢ N2(g) + O2(g)+NO2(g), AH; = 33.2 kJ 2. N2(g) + O2(g) NO(g), AHB = 90.2 kJ 1. When two reactions are added, their enthalpy values are...
For the reaction: B2O3 + 3H2O 3O2 +B2H6 H=2035KJ How much energy is needed to react excess B2O3 with 25.0 g of H2O
Consider the reaction B2H6(g)+O2(g)=B2O3(s)+3H2O(g) delta heat -2035 kJ/mol calculate the amount of heat released when 24.8g of diaborane is burned heat released=
Consider the two reactions. 2NH3(g)+3N2O(g)4NH3(g)+3O2(g)⟶4N2(g)+3H2O(l)⟶2N2(g)+6H2O(l) Δ?∘=−1010 kJΔ?∘=1531 kJ2NH3(g)+3N2O(g)⟶4N2(g)+3H2O(l) ΔH∘=−1010 kJ4NH3(g)+3O2(g)⟶2N2(g)+6H2O(l) ΔH∘=1531 kJ Using these two reactions, calculate and enter the enthalpy change for the reaction below. N2(g)+12O2(g)⟶N2O(g)N2(g)+12O2(g)⟶N2O(g)
Calculate the standard enthalpy of formation of liquid water (H2O) using the following thermochemical information: 2 B2O3(s) 4 B(s) + 3 O2(g) H = +2509.1 kJ B2O3(s) + 3 H2O(l) B2H6(g) + 3 O2(g) H = +2147.5 kJ 2 B(s) + 3 H2(g) B2H6(g) H = +35.4 kJ H = ______ kJ
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
CHEMWORK Consider the reaction B2H6(g) +3 02(g) → B2O3(s) + 3 H2O(g) AH = -2035 kJ How much heat is released when a mixture of 8.26 g B2H7 and 8.80 g 02 is burned? heat released = kJ Submit Show Hints
A chemist measures the enthalpy change ΔH during the following reaction: 2KCl (s) + 3O2 (g) → 2KClO3 (s) ΔH=78.kJ Use this information to calculate ΔH in kJ for the following reactions: 6KCls + 9O2g → 6KClO3s 2KClO3s → 2KCls + 3O2g 4KClO3s → 4KCls + 6O2g