Calculate the Hrxnfor the following reaction using the provided Hf values. Describe the flow of energy in the reaction based on the value you calculate. C2H2(g)+(5/2)O2(g)->2CO2(g)+H2O(g)
Hf(kJ/mol) |
|
C2H2(g) |
227.0 |
CO2(g) |
-393.5 |
H2O(g) |
-241.8 |
O2(g) |
0 |
Why is the enthalpy change considered a state function? How does this relate to Hess’s Law?
For an endothermic reaction, circle the correct sign of q_cal, q_soln, and q_rxn. Justify your answer for each.
q_cal: positive/negative: Why?
q_soln: positive/negative: Why?
q_rxn: positive/negative: Why?
Calorimeters are not perfect insulators. What does that mean? How do we, as scientists, account for imperfect insulation?
Solution:
>>>For the given reaction,
C2H2(g) + 5/2 O2(g) = 2CO2 (g) + H2O(g)
ΔHrxn = Hf (products) - Hf (reactants)
= 2 mol x Hf (CO2) + 1 mol x Hf (H2O) - 1 mol x Hf (C2H2) - 5/2 mol x Hf (O2)
= 2 mol x (-393.5) kJ/mol + 1 mol x (-241.5) kJ/mol - 1 mol x 227 kJ/mol - 5/2 mol x 0 kJ/mol
= (-787 kJ - 241.5 kJ - 227 kJ + 0 kJ)
= -1255.5 kJ
>>> Enthalpy change is considered as state function becuase it delends upon initial and final states of the system. Since it is calculated by substracting reactants enthalpies from product enthalpies.
>>> For endothermic reaction,
qcal = positive
q sol = positive
q rxn = positive
In all the cases, heat is absorbed which indicates the endothermic reaction.
Calculate the Hrxnfor the following reaction using the provided Hf values. Describe the flow of energy...
Using the standard heats of formation that follow, calculate the standard enthalpy change for the following reaction. Species ΔΗΡ(kJ/mol) CO2(g) -393.5 C2H2(g) 226.7 H2O(g)241.8
Consider the following reaction: C2H2 (g)+ O2 (g) → 2 CO2 (g) + H2O (g) Given of CO2 (g) = -393.5 KJ/mol, H2O (g) = -241.8 KJ/mol, and for C2H2 (g) = 227.4 KJ/mol, calculate for this reaction. How many KJ of heat is released when 0.440 kg of carbon dioxide produced?
Consider the following reaction: C2H2 (g)+ 52 O2 (g) ® 2 CO2 (g) + H2O (g) Given ΔHf° of CO2 (g) = -393.5 KJ/mol, ΔHf° H2O (g) = -241.8 KJ/mol, and ΔHf° for C2H2 (g) = 227.4 KJ/mol, calculate ΔHrxn° for this reaction. How many KJ of heat is released when 0.440 kg of carbon dioxide produced?
Question 16 of 20 Submit Using the provided table, determine the enthalpy for the reaction C3H2 (g) + 5 O2 (g) → 3 CO2 (g) + 4 H2O (g) Substance AHF (kJ/mol) C3H8 (9) -108.4 O2 (9) CO2 (g) -393.5 H2O (9) -241.8
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