The decomposition of N 2 O 5 (g)to NO 2 (g)and O 2 (g)obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 $\times$ 10 - 5 s - 1 at 25°C,what is the initial rate of reaction at 25°C where [N 2 O 5 ] 0 = 8.2 $\times$ 10 - 2 M?

The Answer of The decomposition of N 2 O 5 (g)to NO 2 (g)and O 2 (g)obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 $\times$ 10 - 5 s - 1 at 25°C,what is the initial rate of reaction at 25°C where [N 2 O 5 ] 0 = 8.2 $\times$ 10 - 2 M?

The decomposition of N 2 O 5 (g)to NO 2 (g)and O 2 (g)obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 $\times$ 10 - 5 s - 1 at 25°C,what is the initial rate of reaction at 25°C where [N 2 O 5 ] 0 = 8.2 $\times$ 10 - 2 M?

The Answer of The decomposition of N 2 O 5 (g)to NO 2 (g)and O 2 (g)obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 $\times$ 10 - 5 s - 1 at 25°C,what is the initial rate of reaction at 25°C where [N 2 O 5 ] 0 = 8.2 $\times$ 10 - 2 M?

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The Decomposition of N₂O₅(g)to NO₂(g)and O₂(g)obeys First-Order Kinetics $\times$ 10^-⁵ S^-¹ at 25°C,what Is the Initial Rate of Reaction

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The decomposition of N₂O₅(g) to NO₂(g) and O₂(g) obeys first-order kinetics.Assuming the form of the rate law is: $The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 \times 10-5 s-1 at 25°C,what is the initial rate of reaction at 25°C where [N2O5]0 = 8.2 \times 10-2 M? A) mol/L·s B) mol/L·s C) mol/L·s D) mol/L·s E) none of these$
Where k = 3.4 $\times$ 10^-⁵ s^-¹ at 25°C,what is the initial rate of reaction at 25°C where [N₂O₅]₀ = 8.2 $\times$ 10^-² M?

A) $The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 \times 10-5 s-1 at 25°C,what is the initial rate of reaction at 25°C where [N2O5]0 = 8.2 \times 10-2 M? A) mol/L·s B) mol/L·s C) mol/L·s D) mol/L·s E) none of these$ mol/L·s
B) $The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 \times 10-5 s-1 at 25°C,what is the initial rate of reaction at 25°C where [N2O5]0 = 8.2 \times 10-2 M? A) mol/L·s B) mol/L·s C) mol/L·s D) mol/L·s E) none of these$ mol/L·s
C) $The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 \times 10-5 s-1 at 25°C,what is the initial rate of reaction at 25°C where [N2O5]0 = 8.2 \times 10-2 M? A) mol/L·s B) mol/L·s C) mol/L·s D) mol/L·s E) none of these$ mol/L·s
D) $The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics.Assuming the form of the rate law is: Where k = 3.4 \times 10-5 s-1 at 25°C,what is the initial rate of reaction at 25°C where [N2O5]0 = 8.2 \times 10-2 M? A) mol/L·s B) mol/L·s C) mol/L·s D) mol/L·s E) none of these$ mol/L·s
E) none of these

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The Decomposition of N2O5(g)to NO2(g)and O2(g)obeys First-Order Kinetics ×\times× 10-5 S-1 at 25°C,what Is the Initial Rate of Reaction

The Decomposition of N₂O₅(g)to NO₂(g)and O₂(g)obeys First-Order Kinetics $\times$ 10^-⁵ S^-¹ at 25°C,what Is the Initial Rate of Reaction