An example of a reaction where ∆G = 0 is H2O(s)→H2O(l) @SATP any reaction that is over H2O(g)→H2O(l) @SATP all combustio...
An example of a reaction where ∆G = 0 is
H2O(s)→H2O(l) @SATP
any reaction that is over
H2O(g)→H2O(l) @SATP
all combustion reactions
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An example of a reaction where ∆G = 0 is H2O(s)→H2O(l) @SATP any reaction that is over H2O(g)→H2O(l) @SATP all combustio...
An example of a reaction where ∆G = 0 is a. any double displacement reaction b....
An example of a reaction where ∆G = 0 is a. any double displacement reaction b. CO2(s)→CO2(g) @SATP c. CO2(s)→CO2(l) @SATP d. any reaction that is done
at SATP, which reaction below is spontaneous NaCl(s) —> NaCl(l) NaCl(l) —> NaCl(s) NaCl(g) —> NaCl(s)...
at SATP, which reaction below is spontaneous NaCl(s) —> NaCl(l) NaCl(l) —> NaCl(s) NaCl(g) —> NaCl(s) NaCl(aq) —> Na+(aq) + Cl- (aq)
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH...
Applying Hess’s Law, from the enthalpies of reactions, 2NaCl(s) + H2O(l) --> 2HCl(g) + Na2O(s) ΔH = + 507.31 kJ NO(g) + NO2(g) + Na2O(s) --> 2NaNO2(s) ΔH = − 427.14 kJ NO(g) + NO2(g) --> N2O(g) + O2(g) ΔH = − 42.68 kJ 2HNO2(l) --> N2O(g) + O2(g) + H2O(l) ΔH = + 34.35 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: HCl(g) + NaNO2(s) --> HNO2(l) + NaCl(s) (You should show work to get credit) 5-Magnesium burns...
Consider the combustion reaction of propane: CzHg(s) + 5O2(g) + CO2(g) + 4 H2O(g), where AH=-2223...
Consider the combustion reaction of propane: CzHg(s) + 5O2(g) + CO2(g) + 4 H2O(g), where AH=-2223 kJ. If 6.70 X 104 kJ of energy is released in the reaction how many moles of water are formed? 0 120.6 moles There is no correct answer O 30.14 moles 0 90.4 moles O 15.07 moles
2. For the following example, identify the following. H2O(l) → H2O(s) question 2 options a negative...
2. For the following example, identify the following.
H2O(l) → H2O(s)
question 2 options
a negative ΔH and a negative ΔS
a positive ΔH and a negative ΔS
a negative ΔH and a positive ΔS
a positive ΔH and a positive ΔS
It is not possible to determine without more information.
3. Calculate ΔS°rxn for the following reaction. The S° for each
species is shown below the reaction.
C2H2(g) + H2(g) →
C2H4(g)
S°(J/mol∙K) 200.9 130.7 219.3
Question 4 options:...
Part A Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) Express your answer in kilojoules...
Part A Determine the enthalpy for this reaction: Ca(OH)2(s)+CO2(g)→CaCO3(s)+H2O(l) Express your answer in kilojoules per mole to one decimal place. ΔHrxn∘= kJ/mol Part B Consider the reaction Ca(OH)2(s)→CaO(s)+H2O(l) with enthalpy of reaction ΔHrxn∘=65.2kJ/mol What is the enthalpy of formation of CaO(s)? Express your answer in kilojoules per mole to one decimal place. ± Enthalpy Enthalpy H is a measure of the energy content of a system at constant pressure. Chemical reactions involve changes in enthalpy, ΔH, which can be measured...
5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water...
5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water is written as HOH(), then the equation is Na(s) + HOH(l) ? NaOH(aq) + H2(g) Write the following reactions: Oxidation reaction: Reduction reaction: Balanced net ionic reaction: Reducing agent: Oxidizing agent:
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The...
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
Consider the following equilibrium reaction: CaCO3 (s) + CO2 (g) + H2O (l) ⇌ 2 HCO3- (aq)...
Consider the following equilibrium reaction: CaCO3 (s) + CO2 (g) + H2O (l) ⇌ 2 HCO3- (aq) + Ca2+ (aq) Which of these species should be included in the equilibrium constant expression (K) for this reaction? Select all that apply A.) Ca2+ (aq) B.) CaCO3 (s) C.) H2O (l) D.) CO2 (g) E.) HCO3- (aq)
For which reaction will Kp = Kc? C(s) + O2(g) ⇌ CO2(g) 2 H2O(l) ⇌ 2 H2(g)...
For which reaction will Kp = Kc? C(s) + O2(g) ⇌ CO2(g) 2 H2O(l) ⇌ 2 H2(g) + O2(g) CaCO3(s) ⇌ CaO(s) + CO2(g) H2CO3(s) ⇌ H2O(l) + CO2(g) 2 HgO(s) ⇌ Hg(l) + O2(g)
Consider the combustion reaction of propane: CzHg(s) + 5O2(g) + CO2(g) + 4 H2O(g), where AH=-2223 kJ. If 6.70 X 104 kJ of energy is released in the reaction how many moles of water are formed? 0 120.6 moles There is no correct answer O 30.14 moles 0 90.4 moles O 15.07 moles
2. For the following example, identify the following.
H2O(l) → H2O(s)
question 2 options
a negative ΔH and a negative ΔS
a positive ΔH and a negative ΔS
a negative ΔH and a positive ΔS
a positive ΔH and a positive ΔS
It is not possible to determine without more information.
3. Calculate ΔS°rxn for the following reaction. The S° for each
species is shown below the reaction.
C2H2(g) + H2(g) →
C2H4(g)
S°(J/mol∙K) 200.9 130.7 219.3
Question 4 options:...
5. Consider the following redox molecular reaction: Na(s) + H2O(l) ? NaOH(aq) + H2(g) If water is written as HOH(), then the equation is Na(s) + HOH(l) ? NaOH(aq) + H2(g) Write the following reactions: Oxidation reaction: Reduction reaction: Balanced net ionic reaction: Reducing agent: Oxidizing agent:
the enthalpy of combustion of CH4(g) to make H2O(l) and CO2(g) is -2340 kJ mol-1. The enthalpy of combustion of CH2(g) to make H2O(l) and CO2(g) is -2760 kJ mol-1. The enthalpy of formation of H2O(l) is -286 kJ mol-1. All the data are for 298 K. The heat capacities for O2(g), CHA(8), CH3(g), H2O(l) and CO2(8) are 29, 61, 71, 75 and 37 JK"mor", respectively. Deduce a) 4U298 for the combustion of C4H8(g). 5) AH for the combustion of...
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