Recent questions in Chemical thermodynamics

0 votes

1 answer 87 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 SusannahCrow (2.4k points)

0 votes

1 answer 85 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 AgnesXyg5256 (2.0k points)

0 votes

1 answer 31 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 WilheminaMea (1.5k points)

0 votes

1 answer 84 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 BradlySyr093 (1.8k points)

0 votes

1 answer 95 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 MarielScully (1.4k points)

0 votes

1 answer 102 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 CarltonWoote (1.7k points)

0 votes

1 answer 82 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 AnnetteYbc3 (1.6k points)

0 votes

1 answer 75 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 MariRosetta0 (2.2k points)

0 votes

1 answer 81 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 JordanHering (2.2k points)

0 votes

1 answer 100 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 FinleySalern (1.6k points)

0 votes

1 answer 76 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 AngeliaDewey (1.8k points)

0 votes

1 answer 70 views

Calculate the Gibbs free energy change for the chemical reaction: 2H2O (l) → 2H2 (g) + O2 (g)at a temperature of 298 K, given that the standard Gibbs free energies of formation are ΔGf°(H2O) = -237.13 kJ/mol, ΔGf°(H2) = 0 kJ/mol, and ΔGf°(O2) = 0 kJ/mol.

asked Jan 23 in Chemical thermodynamics by ShaunteYun90 (1.4k points)

0 votes

1 answer 75 views

Calculate the Gibbs free energy change at standard conditions for the reaction:2 H2(g) + O2(g) → 2 H2O(l)Given: ΔHºf[H2O(l)] = -285.8 kJ/mol, ΔHºf[H2(g)] = 0 kJ/mol, ΔHºf[O2(g)] = 0 kJ/mol, and ΔSº[H2O(l)] = -69.9 J/K·mol.

asked Jan 23 in Chemical thermodynamics by ChauFrederic (1.2k points)

0 votes

1 answer 109 views

Calculate the Gibbs free energy change at standard conditions for the combustion of propane:C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) Given the standard enthalpy of formation data: ΔH°f(CO2(g)) = -393.5 kJ/mol ΔH°f(H2O(l)) = -285.8 kJ/mol ΔH°f(C3H8(g)) = -103.85 kJ/mol and the standard entropy data: S°(CO2(g)) = 213.6 J/(mol•K) S°(H2O(l)) = 69.9 J/(mol•K) S°(C3H8(g)) = 269.9 J/(mol•K)

asked Jan 23 in Chemical thermodynamics by CWDKristeen0 (1.7k points)

0 votes

1 answer 84 views

Calculate the Gibbs free energy change at 298 K for the reaction of hydrogen gas (H2) and chlorine gas (Cl2) to form hydrogen chloride gas (2HCl), given the following thermodynamic data:∆H°f (HCl) = -92.31 kJ/mol∆H°f (H2) = 0 kJ/mol∆H°f (Cl2) = 0 kJ/mol∆S°f (HCl) = -181.6 J/(mol*K)∆S°f (H2) = 130.7 J/(mol*K)∆S°f (Cl2) = 223.1 J/(mol*K)Also, determine whether the reaction is spontaneous at 298 K and if it will shift towards products or reactants.

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

0 votes

1 answer 96 views

Calculate the Gibbs free energy change at 25°C for the reaction:2NO(g) + O2(g) → 2NO2(g)Given the standard Gibbs free energy of formation at 25°C for NO(g), O2(g), and NO2(g) are +86.4 kJ/mol, 0 kJ/mol, and +51.3 kJ/mol, respectively.

asked Jan 23 in Chemical thermodynamics by GroverRamey (2.2k points)

0 votes

1 answer 71 views

Calculate the Gibbs free energy change (ΔG) for the reaction:N2(g) + 3H2(g) ⇌ 2NH3(g)Given the standard Gibbs free energy of formation (ΔG°f) values at 298 K are:ΔG°f of NH3(g) = -16.6 kJ/molΔG°f of N2(g) = 0 kJ/molΔG°f of H2(g) = 0 kJ/molAssume ideal gas behavior for all gases involved in the reaction.

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

0 votes

1 answer 75 views

Calculate the Gibbs free energy change (ΔG) for the reaction below at 298 K given the following standard Gibbs free energy of formation data: 2H2(g) + O2(g) → 2H2O(l) ΔG°f (kJ/mol): H2(g) = 0 O2(g) = 0 H2O(l) = -237.14

asked Jan 23 in Chemical thermodynamics by ShanicePeele (2.0k points)

0 votes

1 answer 99 views

Calculate the Gibbs free energy change (ΔG) for the following chemical reaction at 25°C and constant pressure of 1 atm:2H2(g) + O2(g) → 2H2O(l)Given the following standard Gibbs free energy of formation values (ΔfG°) at 25°C:H2(g) = 0 kJ/molO2(g) = 0 kJ/molH2O(l) = -237 kJ/mol

asked Jan 23 in Chemical thermodynamics by KraigHogue46 (1.8k points)

0 votes

1 answer 80 views

Calculate the Gibbs free energy change (∆G) for the combustion of methane, CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l), at standard conditions (298 K and 1 atm pressure) using appropriate thermodynamic data.

asked Jan 23 in Chemical thermodynamics by FerminRosale (1.5k points)

Recent questions in Chemical thermodynamics

Categories