Recent questions in Chemistry

0 votes

1 answer 45 views

Calculate the heat capacity of 50 grams of water at 25°C, given that the specific heat capacity of water is 4.18 J/g°C.

asked Jan 23 in Chemical thermodynamics by Leatha15H194 (350 points)

0 votes

1 answer 48 views

Calculate the heat capacity of 50 grams of pure water at 25°C, given that the specific heat capacity of water is 4.184 J/g°C.

asked Jan 23 in Chemical thermodynamics by LouiePickett (490 points)

0 votes

1 answer 49 views

Calculate the heat capacity of 25 grams of liquid ethanol at 25°C when it is heated from 25°C to 35°C by absorbing 150 Joules of heat. The specific heat of ethanol is 2.44 J/g°C.

asked Jan 23 in Chemical thermodynamics by YongTherry1 (450 points)

0 votes

1 answer 12 views

Calculate the heat capacity of 25 grams of aluminum if it was heated from 25°C to 100°C and absorbed 750 Joules of heat energy.

asked Jan 23 in Chemical thermodynamics by SterlingOrne (410 points)

0 votes

1 answer 50 views

Calculate the heat capacity of 10 grams of water if the temperature of the water increases by 5°C upon absorption of 200 Joules of heat.

asked Jan 23 in Chemical thermodynamics by TysonMacnama (770 points)

0 votes

1 answer 56 views

Calculate the heat capacity of 10 grams of water at 25°C if it requires 500 joules of heat to raise its temperature by 5°C.

asked Jan 23 in Chemical thermodynamics by AngelikaNoac (350 points)

0 votes

1 answer 33 views

Calculate the heat absorbed or released during the crystallization of 50g of sodium acetate from a solution if the enthalpy change of the process is -3.9 kJ/mol.

asked Jan 23 in ThermoChemistry by CrystalAshe (560 points)

0 votes

1 answer 54 views

Calculate the heat (in kJ/mol) evolved when 1 mole of hydrogen gas is adsorbed on a surface if the enthalpy of adsorption for hydrogen is -30 kJ/mol.

asked Jan 23 in ThermoChemistry by KandyApplega (310 points)

0 votes

1 answer 61 views

Calculate the Gibbs free energy change for the reaction: 2H2(g) + O2(g) → 2H2O(g) at standard conditions (298 K and 1 atm pressure) given the following data:ΔH˚f[H2O(g)] = -241.8 kJ/molΔH˚f[H2(g)] = 0 kJ/molΔH˚f[O2(g)] = 0 kJ/molΔS˚[H2(g)] = 130.7 J/K·molΔS˚[O2(g)] = 205.0 J/K·molΔS˚[H2O(g)] = 188.8 J/K·mol

asked Jan 23 in Chemical thermodynamics by GraceHershbe (430 points)

0 votes

1 answer 40 views

Calculate the Gibbs free energy change for the following reaction at 298 K:2CH4(g) + 3O2(g) → 2CO2(g) + 2H2O(g)Given the standard Gibbs free energy of formation at 298 K for CH4(g), O2(g), CO2(g) and H2O(g) are -50.8 kJ/mol, 0 kJ/mol, -394.4 kJ/mol, and -241.8 kJ/mol respectively.

asked Jan 23 in Chemical thermodynamics by AlicaOrmond1 (430 points)

0 votes

1 answer 53 views

Calculate the Gibbs free energy change for the following reaction at 298 K: 2H2(g) + O2(g) → 2H2O(l) Given, ΔH = -483.6 kJ/mol and ΔS = -109.4 J/K/mol.

asked Jan 23 in Chemical thermodynamics by ReganHannam5 (370 points)

0 votes

1 answer 39 views

Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)Given:Standard Gibbs free energy change of formation of Mg2+: -466 kJ/molStandard Gibbs free energy change of formation of H+: 0 kJ/molStandard Gibbs free energy change of formation of H2: 0 kJ/molStandard Gibbs free energy change of formation of Mg: 0 kJ/mol

asked Jan 23 in ElectroChemistry by BobRiv48789 (370 points)

0 votes

1 answer 46 views

Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:2Fe³⁺(aq) + 2e⁻ → 2Fe²⁺(aq)Given that the standard Gibbs energy of formation of Fe³⁺(aq) is -290.5 kJ/mol and that of Fe²⁺(aq) is -91.2 kJ/mol.

asked Jan 23 in ElectroChemistry by JorgDesir647 (660 points)

0 votes

1 answer 47 views

Calculate the Gibbs Free Energy change for the following chemical reaction at 298 K:2H2(g) + O2(g) → 2H2O(l) Given the standard Gibbs free energy of formation values: ΔGf°[H2(g)] = 0 kJ/molΔGf°[O2(g)] = 0 kJ/molΔGf°[H2O(l)] = -237 kJ/mol

asked Jan 23 in Chemical thermodynamics by ChristianeTy (570 points)

0 votes

1 answer 58 views

Calculate the Gibbs free energy change for the electrochemical reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Given the standard reduction potentials: E°(Cu2+/Cu) = 0.34 V E°(Zn2+/Zn) = -0.76 V Assuming standard conditions of 1 M concentration and 1 atm pressure at 25°C.

asked Jan 23 in ElectroChemistry by AbrahamMaruf (550 points)

0 votes

1 answer 40 views

Calculate the Gibbs free energy change for the electrochemical reaction where zinc metal (Zn) is oxidized by aqueous hydrogen ions (H+) to form aqueous zinc ions (Zn2+) and hydrogen gas (H2) at 298 K, given that the standard reduction potential of Zn2+/Zn is -0.76 V and the standard hydrogen electrode potential is 0 V.

asked Jan 23 in ElectroChemistry by ZVSLourdes7 (590 points)

0 votes

1 answer 49 views

Calculate the Gibbs free energy change for the electrochemical reaction where Fe(s) is oxidized to Fe3+(aq) and Br2(l) is reduced to Br-(aq) with the help of the following half-reactions: Fe3+(aq) + e- ⇌ Fe2+(aq) E° = 0.771 VBr2(l) + 2e- ⇌ 2Br-(aq) E° = 1.087 V

asked Jan 23 in ElectroChemistry by BennieFll738 (410 points)

0 votes

1 answer 54 views

Calculate the Gibbs free energy change for the electrochemical reaction in which 2 moles of electrons are transferred from a zinc electrode to a copper electrode. The standard reduction potentials are E°(Cu²⁺/Cu) = 0.34 V and E°(Zn²⁺/Zn) = -0.76 V. What is the spontaneity of the reaction under standard conditions?

asked Jan 23 in ElectroChemistry by EloyHakala8 (330 points)

0 votes

1 answer 56 views

Calculate the Gibbs free energy change for the combustion of methane gas to produce carbon dioxide and water vapor at a temperature of 298K and a pressure of 1 atm, given the equation:CH4(g) + 2O2(g) -> CO2(g) + 2H2O(g) ΔG°f = -394.36 kJ/mol (CO2); ΔG°f = -237.13 kJ/mol (H2O); ΔG°f = -50.8 kJ/mol (CH4); ΔG°f = 0 kJ/mol (O2)

asked Jan 23 in Chemical thermodynamics by Steve6884784 (630 points)

0 votes

1 answer 39 views

Calculate the Gibbs free energy change for the combustion of ethane gas in oxygen gas to form carbon dioxide gas and water vapor at a temperature of 25 °C and a pressure of 1 atm, given the following thermodynamic data:Reaction: C2H6(g) + 3.5O2(g) → 2CO2(g) + 3H2O(g)ΔH°rxn = -1560.8 kJ/molΔS°rxn = -283.3 J/K•molUsing the above information, what is the value of the Gibbs free energy change at standard conditions?

asked Jan 23 in Chemical thermodynamics by KermitGodoy (330 points)

Categories