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?

2b2t

explanation:

2b2t

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24

its pwirhfpiwe

explanation:

because dgjpwojefopjwp