Homework Answers
In exothermic reaction, heat is produced.
So, there should be +heat in product.
If heat is in reactant, this is endothermic reaction
Answer: option 1, 2, 5, 6
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Which of the reactions are exothermic? 2 Mg(s) + 0, (g) 2 MgO(s) + heat NH,...
Which of the reactions are exothermic? 2Mg(s)+O2(g)⟶2MgO(s)+heat2Mg(s)+O2(g)⟶2MgO(s)+heat NH3(g)+HCl(g)⟶NH4Cl(s)+heatNH3(g)+HCl(g)⟶NH4Cl(s)+heat AgCl(s)+heat⟶Ag+(aq)+Cl−(aq)AgCl(s)+heat⟶Ag+(aq)+Cl−(aq) 2Fe2O3(s)+3C(s)+heat⟶4Fe(s)+3CO2(g)2Fe2O3(s)+3C(s)+h
Which of the reactions are exothermic? 2Mg(s)+O2(g)⟶2MgO(s)+heat2Mg(s)+O2(g)⟶2MgO(s)+heat NH3(g)+HCl(g)⟶NH4Cl(s)+heatNH3(g)+HCl(g)⟶NH4Cl(s)+heat AgCl(s)+heat⟶Ag+(aq)+Cl−(aq)AgCl(s)+heat⟶Ag+(aq)+Cl−(aq) 2Fe2O3(s)+3C(s)+heat⟶4Fe(s)+3CO2(g)2Fe2O3(s)+3C(s)+heat⟶4Fe(s)+3CO2(g) C(graphite)+O2(g)⟶CO2(g)+heatC(graphite)+O2(g)⟶CO2(g)+heat CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)+heat
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) ...
Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: (0.25 pt.) Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol,...
balance this equ Mg(s) + N2(g) + O2(g) → MgO(s) + Mg3N2(s) MgO(s) + Mg3N2(s) +...
balance this equ Mg(s) + N2(g) + O2(g) → MgO(s) + Mg3N2(s) MgO(s) + Mg3N2(s) + H2O(l) → MgO(s) + Mg(OH)2 (s) + NH3(g) MgO(s) + Mg(OH)2 (s) → MgxOy(s) + H2O(g)
tion 12 of 12 > Attempt 4 When 0.813 g of sodium metal is added to...
tion 12 of 12 > Attempt 4 When 0.813 g of sodium metal is added to an excess ofhydrochloric acid, 8450 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) +2 HCl(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: kJ TOOLS x10 contact us help privacy policy terms of use about us careers MacBook Pro When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. Attempt 2...
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g)...
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g) + 1/2O2(g) → H2O(1) AH = -286 kJ/mol (5) Mg(s) + 2 HCl(aq) → MgCl(aq) + Halg) Hºex (5)= -554 kJ/mol (6) MgO(s) + 2 HCl(aq) → MgCl(aq) + H2O(1) Hev(6) = -193 kJ/mol Calculate AHx(7) for the goal reaction: Mg(s) + 1/2 0.(g) → MgO(s) and show your work. AH'expe() = kJ/mol Calculate the percent error in your calculated value for the above...
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------>...
a) Using the Hess Law and the thermochemical equations below, MgO(s) + + 2HCl(aq) ------> MgCl2(g) + H2O(l) ΔHrxn = -111.7 kJ/mol Mg(s) + 2 HCl(aq) ------> MgCl2(g) + H2(g) ΔHrxn = -548.3 kJ/mol H2(g) + 1/2 O2(g) ------> H2O(l) ΔHrxn = -142.9 kJ/mol find the heat of reaction of the following: Mg(s) + 1/2 O2(g) ------> MgO(g) ΔHrxn = ? b) If the theoretical enthalpy of this reaction is -602 kJ/mol, calculate the percent error
Which reaction or process has the greatest positive change in entropy, AS? A. 2 SO2(g) +...
Which reaction or process has the greatest positive change in entropy, AS? A. 2 SO2(g) + O2(g) - 2 SO3(g) B. 2 KCIO3(s) - 2 KCl(s) + 3 O2(g) C. 2 Mg(s) + O2(E) – 2 Mgo(s) OD.2 C2H2(g) +5 O2(g) – 4 CO2(g) + 2 H20(1) E. Ag+(aq) + Cit(aq) – AgCl(s)
(Before you do the experiment) review, in the following equations for familiar reactions, write an R over the red...
(Before you do the experiment) review, in the following equations for familiar reactions, write an R over the reducing agent and an over sent At the right, indicate the change in oxidation mumber per atom for each element whose oxidation number changes. If there is no change, write in "no change in oxidation number Element oxidized Oxidation number increase per atom Oxidation number decrease per atom Element reduced Reaction 2 Al(s) + 3 Cl2(g) → 2 A13+ + 6 CI-...
Which of the reactions are exothermic? W\ce{2Mg (s) +0_2(g) -> 2MgO (8) }{\quad \quad \quad \quad\quad...
Which of the reactions are exothermic? W\ce{2Mg (s) +0_2(g) -> 2MgO (8) }{\quad \quad \quad \quad\quad quad-www- \Delta H=-1203\text{ kJ/mol}} W) W\e{NH_3 (g) +HCI (g) -> NH_4 CI (8) }{\quad \quad\quad quad quad quad--- \Delta H-176\text{ kJ/mol]) W\e{AgCl (s)-> Ag^+ (aq) +CI^- (aq) }{\quad\quad \quad \quad \quad \quad \Delta H=127\text{ kJ/mol}} W \ce[2Fe_20_3 (s) +3C (s) -> 4Fe (s) +3CO_2 (8) }{\quad\quad-- \Delta H=468\text{ kJ/mol}} \) W\e{C (graphite) +0_2(g) -> 00_2(g) }{\quad \quad\quadquad\quad quad-- \Delta H=-393.5\text{ kJ/mol}} W\e{CH_4 (8) +20_2...
1. Which reaction(s) is/are exothermic? Select all that apply. ΔHf° in kJ/mol at 25°C MgO -601...
1. Which reaction(s) is/are exothermic? Select all that apply. ΔHf° in kJ/mol at 25°C MgO -601 Fe2O3(s) -824 Ag2O (s) -31 Al2O3(s) -1676 Group of answer choices a. 6Ag(s) + Fe2O3(s) --> 3Ag2O(s) + 2Fe(s) b. 2Al(s) + Fe2O3(s) --> Al2O3(s) + 2Fe(s) c. 3Mg(s) + Fe2O3(s) --> 3MgO(s) + 2Fe(s) 2. Which metal requires the most energy to extract (i.e. return to it's metallic form) from it's ore? Reaction ΔHf° kJ/mol metal oxide 2Au(s) + 3/2 O2(g) --> Au2O3(s)...
tion 12 of 12 > Attempt 4 When 0.813 g of sodium metal is added to an excess ofhydrochloric acid, 8450 J of heat are produced. What is the enthalpy of the reaction as written? 2 Na(s) +2 HCl(aq) 2 NaCl(aq) + H2(g) Enthalpy of reaction: kJ TOOLS x10 contact us help privacy policy terms of use about us careers MacBook Pro When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. Attempt 2...
Part 11: Calculating the enthalpy of formation of MgO(s) Fill in the missing value (4) Ha(g) + 1/2O2(g) → H2O(1) AH = -286 kJ/mol (5) Mg(s) + 2 HCl(aq) → MgCl(aq) + Halg) Hºex (5)= -554 kJ/mol (6) MgO(s) + 2 HCl(aq) → MgCl(aq) + H2O(1) Hev(6) = -193 kJ/mol Calculate AHx(7) for the goal reaction: Mg(s) + 1/2 0.(g) → MgO(s) and show your work. AH'expe() = kJ/mol Calculate the percent error in your calculated value for the above...
Which reaction or process has the greatest positive change in entropy, AS? A. 2 SO2(g) + O2(g) - 2 SO3(g) B. 2 KCIO3(s) - 2 KCl(s) + 3 O2(g) C. 2 Mg(s) + O2(E) – 2 Mgo(s) OD.2 C2H2(g) +5 O2(g) – 4 CO2(g) + 2 H20(1) E. Ag+(aq) + Cit(aq) – AgCl(s)
(Before you do the experiment) review, in the following equations for familiar reactions, write an R over the reducing agent and an over sent At the right, indicate the change in oxidation mumber per atom for each element whose oxidation number changes. If there is no change, write in "no change in oxidation number Element oxidized Oxidation number increase per atom Oxidation number decrease per atom Element reduced Reaction 2 Al(s) + 3 Cl2(g) → 2 A13+ + 6 CI-...
Which of the reactions are exothermic? W\ce{2Mg (s) +0_2(g) -> 2MgO (8) }{\quad \quad \quad \quad\quad quad-www- \Delta H=-1203\text{ kJ/mol}} W) W\e{NH_3 (g) +HCI (g) -> NH_4 CI (8) }{\quad \quad\quad quad quad quad--- \Delta H-176\text{ kJ/mol]) W\e{AgCl (s)-> Ag^+ (aq) +CI^- (aq) }{\quad\quad \quad \quad \quad \quad \Delta H=127\text{ kJ/mol}} W \ce[2Fe_20_3 (s) +3C (s) -> 4Fe (s) +3CO_2 (8) }{\quad\quad-- \Delta H=468\text{ kJ/mol}} \) W\e{C (graphite) +0_2(g) -> 00_2(g) }{\quad \quad\quadquad\quad quad-- \Delta H=-393.5\text{ kJ/mol}} W\e{CH_4 (8) +20_2...
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