Recent questions in Chemistry

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Calculate the heat of combustion for propane gas, C3H8(g), if 12.5 grams of propane are completely burned in excess oxygen gas and the products of reaction are cooled from 700°C to 25°C. The heat capacities of the reactants and products are as follows: C3H8(g): cp = 44.10 J/K O2(g): cp = 29.38 J/K CO2(g): cp = 36.8 J/K H2O(g): cp = 33.6 J/K Assume that the heat capacities of the products and reactants are constant over the temperature range of the reaction and that the heat lost to the surroundings is negligible.

asked Jan 23 in ThermoChemistry by NanVanwagene (1.8k points)

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Calculate the heat of adsorption of hydrogen gas on a platinum surface given the initial temperature of the system is 298 K and the final temperature is 330 K. The mass of the platinum surface used is 5 grams, and the amount of hydrogen adsorbed is 0.01 moles. Assume the heat capacity of the system is constant at 25 J/K.

asked Jan 23 in ThermoChemistry by RobertoMundy (1.7k points)

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1 answer 71 views

Calculate the heat energy required to sublime 25 grams of dry ice (CO2) at -78.5 °C, given the heat of sublimation for CO2 is 573 kJ/mol.

asked Jan 23 in ThermoChemistry by EttaKee54894 (2.1k points)

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1 answer 54 views

Calculate the heat capacity of a 50g sample of water that is heated from 25°C to 45°C, given that the specific heat capacity of water is 4.184 J/g°C.

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

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1 answer 68 views

Calculate the heat capacity of a 25.0 g sample of copper, given that it was heated from 25°C to 50°C when it absorbed 209 J of heat. The specific heat capacity of copper is 0.385 J/g°C.

asked Jan 23 in Chemical thermodynamics by CornellNicho (2.1k points)

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1 answer 64 views

Calculate the heat capacity of 50g of water when its temperature is raised from 25°C to 65°C.

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

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1 answer 64 views

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

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

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1 answer 69 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 Precious09K0 (2.0k points)

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1 answer 55 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)

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1 answer 64 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)

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1 answer 20 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)

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1 answer 71 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)

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1 answer 70 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)

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1 answer 48 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 JodieGartrel (1.8k points)

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1 answer 70 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 JeremiahMoli (1.7k points)

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1 answer 72 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)

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1 answer 61 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)

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1 answer 66 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)

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1 answer 46 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 BarrettGriff (2.0k points)

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1 answer 62 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 JordanChun58 (2.3k points)

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