Given the thermochemical equations   A(g)⟶B(g).      Δ?=90 kJ   B(g)⟶C(g).       Δ?=−110 kJ     find the enthalpy changes for each reaction. 3A(g)⟶3B(g).       Δ?=            kJ     B(g)⟶A(g)            Δ?=           kJ     A(g)⟶C(g)          Δ?=.            kJ

calculate the standard enthalpy of reaction for the imaginary reaction XxA2(g) + 2 Z2(I) --> XxZ4(g) + 2 A(g) ▲H°rxn=?? use the following information and give your answer to 0 decimal places substance standard enthalpy of formation (▲Hf°)

What is the change in enthalpy for the reaction: 2B (s) + 3H2(g) → B2H6 (g) given these thermochemical equations? B2H6 (g) + 302 (g) →B2O3 (s) + 3 H₂O (g) AH = -2032 kJ 2B (s) + 3/2 O2 (g) → B2O3 (s) AH = -1272 kJ H2(g) + 1/2 O2 (g) → H2O (g) AH -241.8 kJ -4029 kJ +518.2 kJ +34.6 kJ -3546 kJ

Using the provided table, determine the enthalpy for the reaction C3H8 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AH¡ (kJ/mol) C3H® (g) -108.4 O2 (g) CO2 (g) -393.5 H2O (g) -241.8

The value of ΔH0for the reaction is -482 kJ.  What is the heat released to the surroundings when 12.0 g of CO (g) reacts completely: 2CO(g) + O2(g) →2CO2(g) in kJ?

When HCl(g) reacts with NH3(g) to form NH4CI(s) , 176 kJ of energy are evolved for each mole of HCl(g) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term (including the units) in the last box on the appropriate side of the equation. If a box is not needed, leave it blank. + + +

Carbon disulfide reacts with chlorine according to the following reaction equation: CS2(g) + 3 Cl2(g) S2 Cl2(g) + CCI4(g) kJ A,H° = -230 mol If 15.0 g of Cl2 (70.906 g/mol) reacts with excess CS2, how much heat is transferred (include any sign needed) for this reaction? Give your answer in kJ but do not put units in the answer box. Report it to two decimal places.