# Can u pls explain me the variation of total pressure of a reaction with time like decomposition of ethylene oxide into CH4 and CO

Dear Student,

For the decomposition of ethylene oxide into methane and carbon monoxide, the reaction is

CH2CH2$\to$   CH4 + CO
1 mole of ethylene oxide decomposes to form 1 mole each of methane and carbon monoxide. So, 1 mole of reactant gives rise to 2 moles of products.
According to the ideal gas equation, at constant temperature and volume, the pressure of a gas is directly proportional to the number of moles of the gas.  As moles of gas increases as reaction proceeds, the total pressure also increases.
For a reaction that has lesser number of moles of products than reactants, the total pressure of the reaction decreases with progress of the reaction. An example of such reaction is, N2 + 3H2 $\to$ 2NH3

Hope this information will clear your doubts about change of total pressure with time for a reaction involving gases.

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Regards

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