You wish to know the enthalpy change for the formation of liquid PCI, from the elements.P.()+6 Cl₂(g) →4 PC (6) A, H-7The enthalpy change for the formation of PCs from the elements can be determined experimentally, as can the enthalpy change for the reaction of PCs (f) withmore chlorine to give PCI, (s):P.()+10 Cl₂(g) 4 PCI, ()A,H-1774.0 kJ/mol-rxnPCI, ()+ Cl₂(g) → PCI, (s)-A,H-123.8 kJ/mol-rxnUse these data to calculate the enthalpy change for the formation of 2.20 mol of PCs (4) from phosphorus and chlorine.Enthalpy change -k3

We have to calculate the enthalpy change for 2.20 mol PCl3(l)

You wish to know the enthalpy change for the formation of liquid PCI, from the elements. Pa (0) +6Ch (g) →4 PC (6) A, H-7 The enthalpy change for the formation of PCI, from the elements can be determined experimentally, as can the enthalpy change for the reaction of PC, (f) with more chlorine to give PCI, (s): P.(0)+10 Cl₂(g) → 4 PCI, () A,H-1774.0 kJ/mol-ran PCI, () + Cl₂(g) → PCI (0) A,H-123.8 kJ/mol-rxn Use these data to calculate the enthalpy change for the formation of 2.20 mol of PCs () from phosphorus and chlorine Enthalpy change -

You wish to know the enthalpy change for the formation of liquid PCI, from the elements. Pa (0) +6Ch (g) →4 PC (6) A, H-7 The enthalpy change for the formation of PCI, from the elements can be determined experimentally, as can the enthalpy change for the reaction of PC, (f) with more chlorine to give PCI, (s): P.(0)+10 Cl₂(g) → 4 PCI, () A,H-1774.0 kJ/mol-ran PCI, () + Cl₂(g) → PCI (0) A,H-123.8 kJ/mol-rxn Use these data to calculate the enthalpy change for the formation of 2.20 mol of PCs () from phosphorus and chlorine Enthalpy change -

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.33QE: The enthalpy change for the following reaction is 393.5 kJ. C(s,graphite)+O2(g)CO2(g) (a) Is energy...

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One step in the manufacturing of sulfuric acid is the conversion of SO2(g) to SO3(g). The thermochemical equation for this process is SO2(g)+12O2(g)SO3(g)H=98.9kJ The second step combines the SO3 with H2O to make H2SO4. (a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g). (b) Is heat absorbed or released in this process?
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?
The enthalpy change for the following reaction is 393.5 kJ. C(s,graphite)+O2(g)CO2(g) (a) Is energy released from or absorbed by the system in this reaction? (b) What quantities of reactants and products are assumed? (c) Predict the enthalpy change observed when 3.00 g carbon burns in an excess of oxygen.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
Calculate the standard enthalpy of combustion for benzene, C6H6. C6H6() + 15/2 O2(g) 6 CO2(g) + 3 H2O() rH = ? The enthalpy of formation of benzene is known [rH[C6H6()] = +49.0 kJ/mol], and other values needed can be found in Appendix L.
Give the definition of the standard enthalpy of formation for a substance. Write separate reactions for the formation of NaCl, H2O , C6H12O6, and PbSO4 that have H values equal to Hf for each compound.