Recent questions in Chemistry

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Calculate the heat of crystallization for NaCl from the given data:The enthalpy of fusion of NaCl = 28.3 kJ/mol and the heat capacity of NaCl is approximately constant at 40.0 J/mol.K for temperatures close to room temperature. The melting point of NaCl is 801 °C and the density of the solid NaCl is 2.16 g/cm³.

asked Jan 23 in ThermoChemistry by ErnestinaB30 (470 points)

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Calculate the heat of crystallization (in kJ/mol) of NaOH if 25g of NaOH dissolves in 100g of water at 25°C and releases 4.75kJ of heat.

asked Jan 23 in ThermoChemistry by GarlandGooge (230 points)

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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 Manie9252773 (410 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 JennieCrumle (230 points)

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1 answer 64 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 HaleyCoulsto (350 points)

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1 answer 49 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 ZitaClymer5 (210 points)

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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 JulietaNesbi (330 points)

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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 LavonFriedma (330 points)

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1 answer 59 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 RoryDelacruz (470 points)

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1 answer 47 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 Francisco19F (370 points)

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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 SantoPortill (350 points)

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1 answer 52 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 SimoneOppen7 (230 points)

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1 answer 14 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 EarthaCockle (430 points)

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1 answer 60 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 BarneyWearne (410 points)

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1 answer 64 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 KristineBund (250 points)

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1 answer 42 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 FranklynSorl (310 points)

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1 answer 56 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 IsidroKump49 (370 points)

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1 answer 69 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 SherylGrice (410 points)

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1 answer 48 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 ArlenRosetta (310 points)

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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 CrystalQob9 (310 points)

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