Recent activity by LorenzoBarra

1 answer 38 views

Calculate the enthalpy change for the complete oxidation of 12.5 g of methane gas assuming that all the heat evolved is used to heat up 150 g of water from 25°C to 35°C. The enthalpy of formation of CH4(g) and H2O(l) are -74.8 kJ/mol and -285.8 kJ/mol, respectively.

asked Jan 23 in ThermoChemistry

1 answer 34 views

Calculate the bond dissociation energy of the carbon-hydrogen bond in methane (CH4), given that the reaction CH4(g) → CH3(g) + H(g) has a ΔH° of 435 kJ/mol.

answered Jan 23 in ThermoChemistry

1 answer 46 views

Assuming standard conditions, calculate the standard enthalpy of combustion of methane (CH4), given that the standard enthalpies of formation of CH4 and H2O are -74.8 kJ/mol and -285.8 kJ/mol, respectively. The balanced chemical equation for the combustion of CH4 is:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) What is the standard enthalpy change (ΔH°) for this reaction?

asked Jan 22 in ThermoChemistry

1 answer 59 views

A galvanic cell consists of a standard hydrogen electrode (SHE) as the cathode and a copper electrode as the anode. The measured potential difference between the two electrodes is 1.23 V. Using Tafel analysis, calculate the anodic and cathodic Tafel slopes for the copper electrode.

asked Jan 22 in ElectroChemistry

1 answer 34 views

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1 answer 47 views

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1 answer 7 views

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1 answer 29 views

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1 answer 15 views

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1 answer 4 views

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1 answer 30 views

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1 answer 28 views

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