Answers by EarlWeiland2

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Calculate the change in enthalpy (ΔH) for the combustion of methane gas (CH4) at 25°C and constant pressure of 1 atm. The equation for the combustion of methane is:CH4 (g) + 2O2 (g) → CO2 (g) + 2H2O (l) Given the standard enthalpies of formation at 25°C are:ΔHf[CH4 (g)] = -74.87 kJ/mol ΔHf[CO2 (g)] = -393.5 kJ/mol ΔHf[H2O (l)] = -285.8 kJ/mol Assume that water is in its liquid phase at the end of the reaction.

answered Jan 23 in Physical Chemistry

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Who was the psychologist that proposed the opponent-process theory of colour vision?

answered Jan 20 in Psychology

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Because they control many cell activities - as well as being controlled by feedback mechanisms - what substances are very important for homeostasis?

answered Dec 30, 2024 in Science

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