Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous.
Calculate \(\Delta \mathrm{H}^{\circ}\) and \(\Delta \mathrm{G}^{\circ}\), using data in Appendix C. Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous.
a) \(\quad 2 P b O(s)+N_{2}(g) \rightarrow 2 P b(s)+2 N O(g)\)
b) \(\mathrm{CS}_{2}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{~S}(g)\)
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Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous.
1. Calculate AH° and AG', using data in Appendix C. Determine whether each reaction is endothermic...
1. Calculate AH° and AG', using data in Appendix C. Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous. a) 2PbO(s) + N2(g) → 2Pb(s) + 2NO(g) b) CS2(1) + 2H20(1) - CO2(g) + 2H,S(9)
Given the following reaction determine (in kJ), and for the following reaction at...
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
Determine whether each reaction indicates an endothermic or an exothermic reaction. Drag the appropriate items to...
Determine whether each reaction indicates an endothermic or an exothermic reaction. Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help AB(1)-A() +B(1) 4NH3(g) +502(g) 4NO(g) + 6H2(gC(s) + H2O(g)-CO() +H,($) energy of reactants = - 184 k1ergy of reactants = -242 kJC(s) + energy of products = - 1086 k malergy of products = - 111 kJ/mot 0,() +CO(g) Exothermic Endothermic
Determine whether each reaction indicates an endothermic or an exothermic reaction Drag the appropriate items to...
Determine whether each reaction indicates an endothermic or an exothermic reaction Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help S02()+ O2(E)SO(8) AB(1)–A(g) +B(I) C(s) + H2O(g) +CO() + H EN,H (1) + 2N,0.(8) N20(g) 21 energy of reactants = –242 ) molenergy of reactants = +60kJ/ energy of products = - 111 k molnergy of products = - 320 kJ Exothermic Endothermic
Given the standard enthalpy changes for the following two reactions: (1) 2C(s) 2H2(g)- AHo 52.3 kJ...
Given the standard enthalpy changes for the following two reactions:(1) \(2 \mathrm{C}(\mathrm{s})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=\mathbf{5 2 . 3} \mathrm{kJ}\)(2) \(2 \mathbf{C}(\mathbf{s})+\mathbf{3 H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{8 4 . 7} \mathrm{kJ}\)what is the standard enthalpy change for the reaction:(3) \(\mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{4}}(\mathbf{g})+\mathbf{H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=?\)Given the standard enthalpy changes for the following two reactions:(1) \(\mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=66.4 \mathrm{~kJ}\)(2) \(2 \mathbf{N}_{2} \mathrm{O}(\mathrm{g}) \longrightarrow \mathbf{2 N}_{2}(\mathbf{g})+\mathbf{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{1 6...
Determine whether the following processes are endothermic or exothermic: Endo or Exothermic? Sign () of AH?...
Determine whether the following processes are endothermic or exothermic: Endo or Exothermic? Sign () of AH? Reaction or Process H1O)H:0(s) H20) H0(g) CH (g) + 20:(g) Co:(g) + 2H :0( ) + heat N:(g)+O:(g)+ heat 2NO(g) If the enthalpy of H2(g) + I2(g) 2HI(g) is equal to +53 of 2HI(g) H2(g) +I2(g)? Explain. k] what is the enthalpy of the reaction mol'
Is water vaporization, H_2O(l) rightarrow H_2O(g), at room temperature and pressure a) exothermic or endothermic? _____...
Is water vaporization, H_2O(l) rightarrow H_2O(g), at room temperature and pressure a) exothermic or endothermic? _____ b) more random or less? _____ c) spontaneous or nonspontaneous? _____ d) work done by the system or to the system? _____
Bond H-H Predict whether the following reactions will be exothermic or endothermic. Reaction A. N. (9)...
Bond H-H Predict whether the following reactions will be exothermic or endothermic. Reaction A. N. (9) + 3H,9 — 2NH, Reaction B. S(g) +0,2) 0,() Reaction C. 2H,09) — 2H,(g) +0,($) Reaction D. 2F(g) — F, (g) N=N AH° (kJ/mol) 432 942 494 155 0=0 F-F H-N 386 459 H-O S=0 522 Which reaction(s) are endothermic? Which reaction(s) are exothermie? D ID OB Strongest bond Weakest bond Answer Bank Si-F Si-I Si-CI
Determine whether each of the following is exothermic or endothermic and indicate the sign of dry ice evaporating...
Determine whether each of the following is exothermic or endothermic and indicate the sign of dry ice evaporating a sparkler burning the reaction that occurs in a chemical cold pack often used to ice athletic injuries Determine whether each of the preceding is exothermic or endothermic. Drag the items into the appropriate bins. Indicate the sign of Delta H Drag the items into the appropriate bins.
A spontaneous reaction Select one: a. is always exothermic. b. may be exothermic or endothermic. c....
A spontaneous reaction Select one: a. is always exothermic. b. may be exothermic or endothermic. c. is always endothermic. d. does not involve any heat exchange with surroundings. Which one? Need help please!
1. Calculate AH° and AG', using data in Appendix C. Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous. a) 2PbO(s) + N2(g) → 2Pb(s) + 2NO(g) b) CS2(1) + 2H20(1) - CO2(g) + 2H,S(9)
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
Determine whether each reaction indicates an endothermic or an exothermic reaction. Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help AB(1)-A() +B(1) 4NH3(g) +502(g) 4NO(g) + 6H2(gC(s) + H2O(g)-CO() +H,($) energy of reactants = - 184 k1ergy of reactants = -242 kJC(s) + energy of products = - 1086 k malergy of products = - 111 kJ/mot 0,() +CO(g) Exothermic Endothermic
Determine whether each reaction indicates an endothermic or an exothermic reaction Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help S02()+ O2(E)SO(8) AB(1)–A(g) +B(I) C(s) + H2O(g) +CO() + H EN,H (1) + 2N,0.(8) N20(g) 21 energy of reactants = –242 ) molenergy of reactants = +60kJ/ energy of products = - 111 k molnergy of products = - 320 kJ Exothermic Endothermic
Given the standard enthalpy changes for the following two reactions:(1) \(2 \mathrm{C}(\mathrm{s})+2 \mathrm{H}_{2}(\mathrm{~g}) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=\mathbf{5 2 . 3} \mathrm{kJ}\)(2) \(2 \mathbf{C}(\mathbf{s})+\mathbf{3 H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{8 4 . 7} \mathrm{kJ}\)what is the standard enthalpy change for the reaction:(3) \(\mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{4}}(\mathbf{g})+\mathbf{H}_{\mathbf{2}}(\mathbf{g}) \longrightarrow \mathbf{C}_{\mathbf{2}} \mathbf{H}_{\mathbf{6}}(\mathbf{g}) \quad \Delta \mathrm{H}^{\circ}=?\)Given the standard enthalpy changes for the following two reactions:(1) \(\mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{NO}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=66.4 \mathrm{~kJ}\)(2) \(2 \mathbf{N}_{2} \mathrm{O}(\mathrm{g}) \longrightarrow \mathbf{2 N}_{2}(\mathbf{g})+\mathbf{O}_{2}(\mathrm{~g}) \quad \Delta \mathrm{H}^{\circ}=-\mathbf{1 6...
Determine whether the following processes are endothermic or exothermic: Endo or Exothermic? Sign () of AH? Reaction or Process H1O)H:0(s) H20) H0(g) CH (g) + 20:(g) Co:(g) + 2H :0( ) + heat N:(g)+O:(g)+ heat 2NO(g) If the enthalpy of H2(g) + I2(g) 2HI(g) is equal to +53 of 2HI(g) H2(g) +I2(g)? Explain. k] what is the enthalpy of the reaction mol'
Is water vaporization, H_2O(l) rightarrow H_2O(g), at room temperature and pressure a) exothermic or endothermic? _____ b) more random or less? _____ c) spontaneous or nonspontaneous? _____ d) work done by the system or to the system? _____
Bond H-H Predict whether the following reactions will be exothermic or endothermic. Reaction A. N. (9) + 3H,9 — 2NH, Reaction B. S(g) +0,2) 0,() Reaction C. 2H,09) — 2H,(g) +0,($) Reaction D. 2F(g) — F, (g) N=N AH° (kJ/mol) 432 942 494 155 0=0 F-F H-N 386 459 H-O S=0 522 Which reaction(s) are endothermic? Which reaction(s) are exothermie? D ID OB Strongest bond Weakest bond Answer Bank Si-F Si-I Si-CI
Determine whether each of the following is exothermic or endothermic and indicate the sign of dry ice evaporating a sparkler burning the reaction that occurs in a chemical cold pack often used to ice athletic injuries Determine whether each of the preceding is exothermic or endothermic. Drag the items into the appropriate bins. Indicate the sign of Delta H Drag the items into the appropriate bins.
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