The gas phase decomposition of ch3chog occurs according to...

The gas-phase decomposition of CH3CHO(g) occurs according to the equation CH3CHO(g) → CH4(g) + CO(g) and is second order. The value of the rate constant is 0.105 M–1s-1 at 490°C. If the concentration of CH3CHO(g) is 0.012 M initially, what will be its concentration 5.0 minutes later?

At 791 K and relatively low pressures, the gas-phase decomposition of acetaldehyde (CH3CHO) is second order in acetaldehyde. CH3CHO (g) → CH4 (g) + CO (g) The total pressure of a particular reaction mixture was found to vary as follows: Time (s) | 0 | 75 | 148 | 308 | 605 Total pressure (atm) | 0.500 | 0.583 | 0.641 | 0.724 | 0.808 a) Use the pressure data to determine the value of the rate constant in units of atm⁻¹s⁻¹. Hint: Determine the partial pressure of CH3CHO that reacted at each time interval and therefore the pressure that remains at each time interval. b) What is the rate constant in the usual units of M⁻¹s⁻¹? Hint: Use the ideal gas law to convert atm⁻¹ to M⁻¹. Ideal gas law is PV = nRT where P = partial pressure (atm), V = volume (L), n = mol, R = ideal gas constant (0.08206 L⋅atm/mol⋅K), T = temperature (K).

Adi S.

Question

The gas-phase decomposition of CH3CHO(g) occurs according to the equation CH3CHO(g) → CH4(g) + CO(g) and is second order. The value of the rate constant is 0.105 M–1s-1 at 490°C. If the concentration of CH3CHO(g) is 0.012 M initially, what will be its concentration 5.0 minutes later?

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