Consider the following reaction for 2NO2(g) + F2(g) → 2NO2F(g). The expression for the rate of reaction interms of the rate of change of partial pressures of reactant and product is/are

Question

Consider the following reaction for 2NO2(g) + F2(g) → 2NO2F(g). The expression for the rate of reaction interms of the rate of change of partial pressures of reactant and product is/are (A) rate = -½[dp(NO2)/dt] (B) rate = ½[dp(NO2)/dt] (C) rate = -½[dp(NO2F)/dt] (D) rate = ½[dp(NO2F)/dt]

Tardigrade Admin · Accepted Answer

2 NO 2(g)+ F 2(g) longrightarrow 2 NO 2 F (g) Rate of reaction =-(1/2)[(d p( NO 2)/d t)] =-[(d p(F2)/d t)] =+(1/2)[(d p( NO 2 F )/d t)]

Q. Consider the following reaction for $2 N O_{2 (g)} + F_{2 (g)} \to 2 N O_{2 F (g)}$ . The expression for the rate of reaction interms of the rate of change of partial pressures of reactant and product is/are

rate $= - ½ [d p (N O_{2}) / d t]$

rate $= ½ [d p (N O_{2}) / d t]$

rate $= - ½ [d p (N O_{2} F) / d t]$

rate $= ½ [d p (N O_{2} F) / d t]$

$2 N O_{2} (g) + F_{2} (g) ⟶ 2 N O_{2} F (g)$
Rate of reaction $= - \frac{1}{2} [\frac{d p ( N O _{2} )}{d t}]$
$= - [\frac{d p ( F _{2} )}{d t}]$
$= + \frac{1}{2} [\frac{d p ( N O _{2} F )}{d t}]$

Q. Consider the following reaction for 2NO2(g)​+F2(g)​→2NO2F(g)​. The expression for the rate of reaction interms of the rate of change of partial pressures of reactant and product is/are

rate =−½[dp(NO2​)/dt]

rate =½[dp(NO2​)/dt]

rate =−½[dp(NO2​F)/dt]

rate =½[dp(NO2​F)/dt]