The first order gaseous decomposition of N2O4 into NO2 has a k value of 45 × 103 s-1 at 1°C and an energy of activation of 58 kJ mol-1 . At what temperature would be 1.00 × 104 s-1 ?

Question

The first order gaseous decomposition of N2O4 into NO2 has a k value of 45 × 103 s-1 at 1°C and an energy of activation of 58 kJ mol-1 . At what temperature would be 1.00 × 104 s-1 ? (A)  274 K  (B)  283 K  (C)  273 K  (D)  293 K

Tardigrade Admin · Accepted Answer

According to Arrhenius equation log (K2/K1) = (Ea/2.303R) ((T2-T1/T1T2)) log (1× 104/4.5 × 103) = (58× 1000 J mol-1/2.3030× 8.314 JK-1 mol-1) × ((T2- 274/274T2)) ⇒ T2 = 2827 ≈ 283 K

Q. The first order gaseous decomposition of $N_{2} O_{4}$ into $N O_{2}$ has a $k$ value of $45 \times 1 0^{3} s^{- 1}$ at $1^{\circ} C$ and an energy of activation of $58 k J m o l^{- 1}$ . At what temperature would be $1.00 \times 1 0^{4} s^{- 1}$ ?

$274 K$

$283 K$

$273 K$

$293 K$

Q. The first order gaseous decomposition of N2​O4​ into NO2​ has a k value of 45×103s−1 at 1∘C and an energy of activation of 58kJmol−1 . At what temperature would be 1.00×104s−1 ?

274K

283K

273K

293K

According to Arrhenius equation logK1​K2​​=2.303REa​​(T1​T2​T2​−T1​​) log4.5×1031×104​ =2.3030×8.314JK−1mol−158×1000Jmol−1​×(274T2​T2​−274​) ⇒T2​=2827≈283K

Q. The first order gaseous decomposition of $N_{2} O_{4}$ into $N O_{2}$ has a $k$ value of $45 \times 1 0^{3} s^{- 1}$ at $1^{\circ} C$ and an energy of activation of $58 k J m o l^{- 1}$ . At what temperature would be $1.00 \times 1 0^{4} s^{- 1}$ ?

$274 K$

$283 K$

$273 K$

$293 K$