The reaction rate can be expressed as the change in the concentration of a produ

Question

The reaction rate can be expressed as the change in the concentration of a product or reactant that occurs over time. The rate of change in the concentration of a reactant has a negative value because reactant concentrations decrease as a reaction proceeds. However, the measured reaction rate is defined as a positive quantity because it describes the rate at which reactants form products, so a minus sign is used with Detla[rectant]/Delta t values to obtain an overall positive value for the reaction rate. Note that the coefficients in front of the terms are the reciprocals of the coefficients in the chemical equations. Given the reaction: 2C_2H_6 (g) + 7O_2 (g) rightarrow 4CO_2 (g) + 6H_2O (g) Express the rate of reaction in terms of the change in concentration of each species. When [O_2] is decreasing at a rate of 0.10 mol.L^-1.S^-1, how fast is [H_2O] increasing? Given the reaction: CO_2 (g) rightarrow CO (g) + 1/2 O_2 (g) Express the rate of reaction in terms of the change in concentration of each species. When [O_2] is increasing at 0.25 moI.L^-1.s^-1, how fast is [CO] increasing?

Explanation / Answer

1. -d[C2H6]/2dt= -d[O2]/(dt*7)= d[CO2]/4dt= d[H2O]/6dt

2, 7, 4 and 6 are stoichiometric coefficients of C2H6, O2, CO2 and H2O respectively.

2. -d[O2]/dt= 0.1 moles/s

but -d[O2]/7dt= d[H2O]/6dt

d[H2O]/dt= (6/7)*0.1= 0.8571 moles/L.se

2. -d[CO2]/dt = d[CO]/dt= 1/2 d[O2]/dt

d[O2]/dt= 0.25 mol/L.s

d[CO]/dt= 1/2 d[O2]/dt

d[CO]/dt =0.25/2 =0.125 mole/L.sec

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