Consider the decomposition of N2)5 in carbon tetrachloride (CCl4) at 45 degrees Celsius. 2N2O5 (aq) ↔ 4NO2 (g) + O2 (g) The reaction is first-order in N2O5 with the specific rate constant 6.08 x 10^-4/s. Calculate the reaction rate at these conditions:
a. [N2O5] = 0.200 mol/L
b. [N2O5] = 0.319 mol/L
2 answers
The first one is supposed to be N2O5
Rate = k[N₂O₅]¹
a. Rate 1 = (6.08 x 10⁻⁴ s⁻¹)(0.200 mol-L⁻¹) = 1.36 x 10⁻⁴ mol/L-s
b. You do ‘b’
a. Rate 1 = (6.08 x 10⁻⁴ s⁻¹)(0.200 mol-L⁻¹) = 1.36 x 10⁻⁴ mol/L-s
b. You do ‘b’
1 answer