Lead(II) oxide can be reduced to form elemental lead through the reaction:\[ \text{PbO}(s) + \text{C}(s) \rightarrow \text{Pb}(s) + \text{CO}(g) \]Calculate \(\Delta H^\circ\) for the above reaction given the following (all values are at \(25^\circ \text{C}\)): **Thermochemical Equation Manipulation**In this example, we will explore how to manipulate thermochemical equations to find the enthalpy change (\( \Delta H^\circ \)) for a given reaction.1. **Reaction Equations and \(\Delta H^\circ\):** - Equation 1: \[ 2 \, \text{CO}(g) + \cancel{\text{O}_2(g)} \rightarrow 2 \, \text{CO}_2(g) \quad \Delta H^\circ = -566.0 \, \text{kJ} \] - Equation 2: \[ 2 \, \text{NO}(g) \rightarrow \text{N}_2(g) + \cancel{\text{O}_2(g)} \quad \Delta H^\circ = -180.5 \, \text{kJ} \]2. **Overall Reaction:** The overall chemical reaction is derived by combining the above equations and eliminating common species on both sides: \[ 2 \, \text{CO}(g) + 2 \, \text{NO}(g) \rightarrow 2 \, \text{CO}_2(g) + \text{N}_2(g) \]3. **Overall Enthalpy Change:** The overall enthalpy change is the sum of the enthalpy changes from each individual reaction: \[ \Delta H^\circ = -746.5 \, \text{kJ} \]This demonstrates the principle of Hess's Law, where the total enthalpy change is the sum of the enthalpy changes of individual steps, allowing you to calculate the enthalpy for a desired reaction from known values.

Interpretation - To determine the the enthalpy of the reaction at 25oC where lead oxide can be reduced to form elemental led through the given reaction . Concept- To determine the enthalpy of the reaction at 25oC here we use the formula - Enthalpy of reaction =∑np∆HProduct - ∑nR∆HReactant Here - np = number of mole of product nR = number of mole of reactant ∆H = enthalpy

Answered: Lead(II) oxide can be reduced to form…

Science

Chemistry

Lead(II) oxide can be reduced to form elemental lead through the reaction: PbO(s) + C(s) → Pb(s) + CO(g) Calculate AH° for the above reaction given the following (all values are at 25°C):

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

8. Nitric oxide reacts with chlorine to form NOCI. The data refer to 298 K. 2NO(g) + Cl₂(g) → 2NOCI(g) Substance: NOCI(g) 51.71 AH° (kJ/mol): 66.07 AG°f(kJ/mol): S°(J/K-mol): 223.0 261.6 What is the value of AG for this reaction at 550 K? Is the reaction spontaneous or not? NO(g) 90.29 86.60 210.65 A) -143.76 kJ, nonspontaneous B) -78.78 kJ, spontaneous C) -22.24 kJ, nonspontaneous D) -10.56 kJ, spontaneous E) 66600 kJ, no idea Cl2₂(g) 0 0
Consider the following reaction; A(g) + B(g)→ c(s) + D(g); AHP = -164.1 kJ; AG = 159.1 kJ at 298 K The reaction is spontaneous at relatively low temperatures only O The reaction is spontaneous at relatively high temperatures only O The reaction is nonspontaneous at all temperatures. O The reaction is at equilibrium at 298 K O The reaction is spontaneous at all temperatures
48 Use data to compute ΔG° at 57.0°C for the following reaction. 2ClO2−(aq) + O2(g) → 2ClO3−(aq) ΔH°f (ClO2−(aq)) = -67 kJ mol-1ΔH°f (ClO3−(aq)) = -104 kJ mol-1ΔS° (ClO2−(aq)) = 101 J mol-1 K-1ΔS° (O2(g)) = 205.152 J mol-1 K-1ΔS° (ClO3−(aq)) = 162 J mol-1 K-1ΔG°f (ClO2−(aq)) = 17 kJ mol-1ΔG°f (ClO3−(aq)) = -3 kJ mol-1
18.45 Using enthalpies of formation (Appendix C), calculate AH° for the following reaction at 25°C. Also calculate AS° for this reaction from standard entropies at 25°C. Use these values to calculate AG° for the reaction at this temperature. 2CH3OH(I) + 302(g) 2CO2(g) + 4H,O(l) -
Consider the following reaction; A(g) + B(g) → c(s) + D(g); AH = 159.1 kJ; AG = 164.1kJ at 298 K %3D The reaction is spontaneous at relatively high temperatures only The reaction is spontaneous at all temperatures The reaction is nonspontaneous at all temperatures. The reaction is at equilibrium at 298 K The reaction is spontaneous at relatively low temperatures only
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 19.35 mm Hg. 2NO(g) + 02(g)→2NO2(g) AG = kJ/mol
14
c) SO d) CO 0. Sodium reacts violently with water according to the equation: 2 Na(s) +2 H;0() 2 NaOH(aq) + H:(g) resulting solution has a higher temperature than the water prior to the addition of sodium. What are the signs of AH and AS for this reaction? a) AH is negative and AS is negative. b) AH is negative and AS is positive. e) AH is positive and AS is negative. d) AH is positive and AS is positive. (END)
For the reaction: CuS (s) + H₂(g) → H₂S (g) + Cu (s) Given: ΔS ⁰ (CuS) = 66.5 J/mole-K ΔHf ⁰ (CuS) = -53.1 kJ/mol ΔS ⁰ (H₂S) = 205 J/ mole-K ΔHf ⁰ (H₂S) = -20.6 kJ/mol ΔS ⁰ (Cu) = 33.3 J/ mole-K ΔH f ⁰ (Cu) = 0.0 kJ/mol ΔS ⁰ (H₂) = 131 J/ mole-K ΔH f ⁰(H₂) = 0.0 kJ/mol The standard free energy of the reaction ΔG ⁰ rxn is A) -37.9 kJ/mole B) 44.6 kJ/mole C) -20.3 kJ/mole D) +20.3kJ/mole and spontaneous E) +37.9 kJ/mole
Calculate AG° at 298 K for the reaction CS, (1) + 30,(g) –→ CO,(g) + 2 SO,(g) based on these reactions. C(s) + 0,(g) Co,(g) AG° = -397.28 kJ/mol S(s) + 0,(g) → so,(g) AG° = -300.19 kJ/mol C(s) +2 S(s) → CS,(1) Cs,(1) AG° = +62.37 kJ/mol AG° = kJ/mol
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(8) + 3H2(g) → 2NH3(g) AG° at 298 K for this reaction is -33.3 kJ/mol. The value of AG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is O -1.8 O -104.5 O-3.86 x 103 O-7.25 x 10 -40.5
A student determines the value of the equilibrium constant to be 1.87x107 for the following reaction. Fe(s) + 2HCI(aq)- →FECI2(s) + H2(g) Based on this value of Keg: AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.39 moles of Fe(s) at standard conditions at 298K. kJ rxn