Recent questions without an upvoted answer

0 votes

1 answer 50 views

Calculate the change in entropy (ΔS) for the reaction in which 3 moles of carbon monoxide (CO) gas is burned with excess oxygen gas to form 3 moles of carbon dioxide (CO2) gas. The reaction is carried out at constant pressure and a temperature of 298 K.

asked Jan 23 in Inorganic Chemistry by QJXClarice2 (2.5k points)

0 votes

1 answer 64 views

Calculate the change in entropy (in J/K) for the following reaction at 298 K: 2CH3OH (l) + 3O2 (g) → 2CO2 (g) + 4H2O (l) Given the following standard entropy values (in J/K): CH3OH (l): 126.6, O2 (g): 205.0, CO2 (g): 213.6, H2O (l): 69.9

asked Jan 23 in Chemical thermodynamics by RondaSkeyhil (1.7k points)

0 votes

1 answer 56 views

Calculate the change in enthalpy for the reaction CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) given that the enthalpies of formation for CH4 (g), CO2 (g) and H2O (l) are -74.81 kJ/mol, -393.51 kJ/mol and -285.83 kJ/mol respectively.

asked Jan 23 in Physical Chemistry by CorneliusBur (2.1k points)

0 votes

1 answer 58 views

Calculate the change in enthalpy for the following chemical reaction: CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l) Given that the enthalpies of formation for CH4(g), CO2(g), and H2O(l) are -74.8 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol respectively.

asked Jan 23 in Chemical reactions by ZKLBarbra368 (2.3k points)

0 votes

1 answer 56 views

Calculate the change in enthalpy for the combustion of 2 moles of methane gas (CH4) at a constant pressure of 1 atmosphere and a temperature of 298 K. Given the standard enthalpy of formation for methane is -74.81 kJ/mol.

asked Jan 23 in Physical Chemistry by JadaMeece33 (1.6k points)

0 votes

1 answer 56 views

Calculate the change in enthalpy and entropy for the reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) at 25°C given the following data:- ΔH°f for MgCl2(aq) = -641.3 kJ/mol- ΔS°f for MgCl2(aq) = -200.9 J/K/mol- ΔH°f for H2(g) = 0 kJ/mol- ΔS°f for H2(g) = 130.7 J/K/mol- ΔH°f for HCl(aq) = -167 kJ/mol- ΔS°f for HCl(aq) = -18.8 J/K/mol- ΔH°f for Mg(s) = 0 kJ/mol- ΔS°f for Mg(s) = 32.7 J/K/molAssume that ΔH°f and ΔS°f are independent of temperature.

asked Jan 23 in Inorganic Chemistry by ArleneLeichh (2.1k points)

0 votes

1 answer 54 views

Calculate the change in enthalpy (ΔH) for the following reaction at 25°C given the standard enthalpies of formation for each compound: 2H2(g) + O2(g) → 2H2O(g) Standard enthalpies of formation: ΔHf° (H2O)(g) = -241.82 kJ/molΔHf° (H2)(g) = 0 kJ/molΔHf° (O2)(g) = 0 kJ/mol

asked Jan 23 in Physical Chemistry by TatianaSteil (2.3k points)

0 votes

1 answer 59 views

Calculate the change in enthalpy (ΔH) for the combustion of methane gas (CH4) at 25°C and constant pressure of 1 atm. The equation for the combustion of methane is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) Given the standard enthalpies of formation at 25°C are:ΔHf[CH4 (g)] = -74.87 kJ/mol ΔHf[CO2 (g)] = -393.5 kJ/mol ΔHf[H2O (l)] = -285.8 kJ/mol Assume that water is in its liquid phase at the end of the reaction.

asked Jan 23 in Physical Chemistry by RobertoLafla (2.1k points)

0 votes

1 answer 61 views

Calculate the change in enthalpy (ΔH) for the combustion of 10 grams of propane (C3H8) if the heat released by the reaction is -2202 kJ.

asked Jan 23 in Chemical reactions by AdelineBurro (1.9k points)

0 votes

1 answer 57 views

Calculate the cell potential for the reaction:Hg2Cl2(s) + 2 Cl-(aq) → 2 Hg(l) + 2 Cl2(g)Given the standard reduction potentials: Hg2Cl2(s) + 2 e- → 2 Hg(l) + 2 Cl-(aq) E° = 0.268 VCl2(g) + 2 e- → 2 Cl-(aq) E° = 1.36 V

asked Jan 23 in ElectroChemistry by FletaStepp73 (2.0k points)

0 votes

1 answer 65 views

Calculate the cell potential for the reaction between a silver electrode and a copper electrode, given that the silver electrode is immersed in a 0.1 M AgNO3 solution and the copper electrode is immersed in a 1.0 M CuSO4 solution at 25°C. (Standard electrode potentials of Ag and Cu electrodes are +0.80 V and +0.34 V, respectively. Carry out the calculation in steps and provide the final answer with appropriate units.)

asked Jan 23 in ElectroChemistry by ChristieJzq (1.7k points)

0 votes

1 answer 48 views

Calculate the cell potential for the following galvanic cell where a nickel anode is placed in a 1.0M Ni(NO3)2 solution and a silver cathode is placed in a 1.0M AgNO3 solution. The balanced equation for the cell reaction is: Ni(s) + 2 Ag+(aq) → Ni2+(aq) +2 Ag(s) Assume that standard reduction potentials for each half-reaction are as follows: Ni2+(aq) + 2 e- ⇌ Ni(s) E° = -0.25V Ag+(aq) + e- ⇌ Ag(s) E° = +0.80V What is the cell potential at standard conditions (25°C and 1 atm)?

asked Jan 23 in ElectroChemistry by GermanFranki (1.8k points)

0 votes

1 answer 61 views

Calculate the cell potential for the following electrochemical reaction:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)Given that the standard reduction potentials for the half-reactions are as follows:Zn2+(aq) + 2e- → Zn(s) E° = -0.76 VCu2+(aq) + 2e- → Cu(s) E° = +0.34 V

asked Jan 23 in ElectroChemistry by TobiasTudawa (1.9k points)

0 votes

1 answer 46 views

Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) The standard reduction potentials are: Cu2+(aq) + 2 e- → Cu(s) E° = 0.34 V Ag+(aq) + e- → Ag(s) E° = 0.80 V

asked Jan 23 in ElectroChemistry by FinleySalern (1.6k points)

0 votes

1 answer 63 views

Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag⁺(aq) → Cu²⁺(aq) + 2 Ag(s) Given that the standard reduction potentials are: Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

asked Jan 23 in ElectroChemistry by AundreaWhitf (1.8k points)

0 votes

1 answer 55 views

Calculate the cell potential for the following electrochemical reaction at 25°C: Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) Given: E°(Ag+/Ag) = +0.80 V E°(Zn2+/Zn) = −0.76 V

asked Jan 23 in ElectroChemistry by Lynell160113 (1.8k points)

0 votes

1 answer 63 views

Calculate the cell potential for a given electrochemical reaction where the half-cell reactions are:* Fe3+(aq) + e- → Fe2+(aq) E° = 0.77 V* Ag+(aq) + e- → Ag(s) E° = 0.80 VAssume 1.0 M solutions and standard state conditions. Determine whether the reaction is spontaneous or non-spontaneous under standard conditions.

asked Jan 23 in ElectroChemistry by AntoniettaLa (1.9k points)

0 votes

1 answer 12 views

Calculate the cell potential at standard conditions for the electrochemical reaction: Cu(s) + 2Ag+(aq) -> 2Ag(s) + Cu2+(aq) given that the standard reduction potentials for Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) are +0.34 V and +0.80 V, respectively.

asked Jan 23 in ElectroChemistry by MoniqueBrins (1.9k points)

0 votes

1 answer 68 views

Calculate the bond order of the nitrogen molecule (N2) using molecular orbital theory.

asked Jan 23 in Physical Chemistry by LorenzoWooll (1.7k points)

0 votes

1 answer 56 views

Calculate the bond order of the molecule NO using molecular orbital theory, given that the nitrogen atom has four valence electrons and the oxygen atom has six valence electrons.

asked Jan 23 in Chemical bonding by Lachlan74F5 (2.0k points)

Recent questions without an upvoted answer

Categories