Part A; Calculate the standard enthalpy change for the reaction
2A+B⇌2C+2D
where the heats of formation are given in the following table:
Substance | ΔH∘f (kJ/mol) |
A | -251 |
B | -375 |
C | 191 |
D | -519 |
Answer to Part A- 221kJ
FIND PART B & C
PART B- For the reaction given in Part A, how much heat is absorbed when 3.40 mol of A reacts?
Express your answer numerically in kilojoules.
PART C- For the reaction given in Part A, ΔS∘rxn is 29.0 J/K . What is the standard Gibbs free energy of the reaction, ΔG∘rxn?
Express your answer numerically in kilojoules.
Many thanks!!!
Substance..ΔH∘f
(kJ/mol)
A.......-251
B...... -375
C... 191
D.... -519
use these numbers to calculate dHrxn of the given reaction
2A+B⇌2C+2D
dHrxn = dH{product}-dH{reactants}
= 2*dH(C) + 2* dH(D) -{ 2*dH(A) + 1*dH(B)}
plug in dH values from the table
dHrxn = {2* (191) +2*(-519)}KJ - { 2(-251) +1* (-375) }KJ
= 221 KJ
***************
the above dHxn is for 2 mole of A ,as per given equatiion
So for 1 mole of A : dHrxn = 221 kj/ 2 = 110.5 KJ
So when we use 3.4 mol of A :
dHrxn = 110.5 KJ* 3.4 mol = 375.7 KJ
***************
given
dS0rxn = 29.0 J/K
dHrxn = 221x10^3 J
standard gibbs energy is calculated using formula
dG0 = dHrxn-TdSrxn
at standard temperature T= 298 K
dG0 = 221 x10^3 j -298 k * 29.0 J/K
= 212.358 KJ
******************************
All solved ,kindly upvote
Part A; Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D where the heats of formation...
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D where the heats of formation are given in the following table: Substance ΔH∘f (kJ/mol) A -275 B -413 C 223 D -521 Express your answer in kilojoules. - Part A Calculate the standard enthalpy change for the reaction 2A+B=2C+2D where the heats of formation are given in the following table: Substance A AH (kJ/mol) -275 -413 223 -521 B D Express your answer in kilojoules. View Available Hint(s) O AED *...
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D where the heats of formation are given in the following table: Substance ΔH∘f (kJ/mol) A -253 B -393 C 205 D -509 Express your answer in kilojoules.
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D where the heats of formation are given in the following table: Substance ΔfH∘ΔfH∘ (kJ mol−1 A −247 B −375 C 187 D −491 For the reaction given in Part A, how much heat is absorbed when 3.30 mol of A reacts? For the reaction in Part A, ΔrS∘=25.0 J K−1 mol−1. What is the standard Gibbs energy of reaction at 297 K , ΔrG∘ (297K)?
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data: Substance ΔH∘f (kJ/mol) A -271 B -381 C 221 D -495 Express your answer in kilojoules.
Part A Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data: Substance ΔH∘f (kJ/mol) A -263 B -409 C 199 D -485 Express your answer to three significant figures and include the appropriate units.
do part b Calculate the standard enthalpy change for the reaction 2A+B=2C+2D Use the following data Substance ΔΗ: (kJ/mol) А -227 B -419 с 195 D -525 Express your answer to three significant figures and include the appropriate units. View Available Hint(s) AH x = 213 kJ Previous Answers ✓ Correct Part B For the reaction given in Part A how much heat is absorbed when 3.20 mol of A reacts? Express your answer to three significant figures and include...
Calculate the standard enthalpy change for the reaction 2A +B ⇌ 2C+2D where the heats of formation are given in the following table:
Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: ΔH∘rxn=ΔH∘f(products)−ΔH∘f(reactants) Entropy change, ΔS∘, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free...
PART A. Calculate the standard enthalpy change for the reaction 2A+B⇌2C+2D Use the following data: Substance ΔH∘fΔHf∘ (kJ/mol)kJ/mol) AA -273 BB -417 CC 223 DD -475 =459kJ PART B. Express your answer to three significant figures and include the appropriate units. For the reaction given in Part A, how much heat is absorbed when 3.80 mol of A reacts? Express your answer to three significant figures and include the appropriate units.