The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled? What is the half-life for a particular reaction if the rate law is rate = (1301 min⁻¹)[A]? Identify the molecularity of the elementary reaction below: 2NO(g) + Br₂(g) → 2NOBr(g)
The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled?
What is the half-life for a particular reaction if the rate law is rate = (1301 min⁻¹)[A]?
Identify the molecularity of the elementary reaction below: 2NO(g) + Br₂(g) → 2NOBr(g)
The following reaction is at equilibrium in a closed 4L vessel: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) What will happen if the vessel volume is reduced to 3L? (Assume constant temperature.)
If Kc = 82 for the reaction below at 200 K, then what is the value of Kp? 2 NO₂ (g) ⇌ N₂O₄ (g)
Consider the reaction: N₂ (g) + 3 Br₂ (g) ⇌ 2 NBr₃ (g) At equilibrium, the concentrations of N₂ and Br₂ are 0.34 M and 0.70 M respectively, and the concentration of NBr₃ is 0.090 M. What is Kc for this equilibrium?
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