Calculate the average kinetic energies of CH4g and N2 g molecules at 273 K and 546K

Chemistry

1 answer:

kaheart [24]2 years ago

7 0

Answer:

Average kinetic energy of gases, which is derived from the RMS (root mean square speed) and KE equation, can be solved as:

It appears that the average KE of gases is dependent on the temperature which means that all gases will have the same KE as long the temperature is the same

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Carbon, hydrogen and ethane each burn exothermically in an excess of air. AHⓇ =-393.7 kJ mol. C(s) + O2(g) → CO2(g) H2(g) + % O2

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Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The chemical equation for the reaction of carbon and water follows:

$2C(s)+2H_2(g)\rightarrow C_2H_4(g)$ $\Delta H^o_{rxn}=?$