Ammonium cyanate (NH4CNO) reacts to form urea (NH2CONH2). at 65 degrees celsius, the rate constant, K is 3.60 L mol^-1 s^-1. what is the rate law for this reaction

v = 3.60Lmol⁻¹s⁻¹ [NH₄CNO]²

Explanation:

The reaction at 65°C of ammonium cyanate to produce urea is:

NH₄CNO → NH₂CONH₂

The general rate law is:

v = K  [NH₄CNO]ˣ

Where v is rate of the reaction, K is rate constant and x represents the order of reaction

Based on the units of the rate constant (Lmol⁻¹s⁻¹ = M⁻¹s⁻¹) the reaction must be order 2 and the rate law:

v = K  [NH₄CNO]²

a electronegativity decreases beacuse the size of nucleus is bigger.