Question

select all of the following reaction conditions that would have an effect of the reaction rate

Given the following balanced chemical reaction: CH4 +202 --> CO2 + 2H20 While the reaction was occurring, the instantaneous rate with respect to CH4 was measured to be -0.025 M CH4/minute. At the same time, the rate with respect to O2 will be __MO2/minute.

Answer 1

Balanced equation of combustion of methane is,

CH4 + 2 O2 -----------> CO2 + 2 H2O

Rate of a reaction can be defined as, "decrease in concentration of reactants or increase in concentration of products per unit time."

Mathematically with respect to reactants,

$rate = - \frac{d[CH_{4}]}{dt} = - \frac{1}{2}\frac{d[O_{2}]}{dt}$

$\frac{d[CH_{4}]}{dt} = \frac{1}{2}\frac{d[O_{2}]}{dt}$

$- 0.025 = \frac{1}{2}\frac{d[O_{2}]}{dt}$

$- 0.025 X 2 = \frac{d[O_{2}]}{dt}$

$\frac{d[O_{2}]}{dt} = 0.050 mol / min$

Answer 2

Balanced equation of combustion of methane is,

CH4 + 2 O2 -----------> CO2 + 2 H2O

Rate of a reaction can be defined as, "decrease in concentration of reactants or increase in concentration of products per unit time."

Mathematically with respect to reactants,

$rate = - \frac{d[CH_{4}]}{dt} = - \frac{1}{2}\frac{d[O_{2}]}{dt}$

$\frac{d[CH_{4}]}{dt} = \frac{1}{2}\frac{d[O_{2}]}{dt}$

-0.025 = 1d02 2 dt

$- 0.025 X 2 = \frac{d[O_{2}]}{dt}$

$\frac{d[O_{2}]}{dt} = 0.050 mol / min$