<p>The overall chemical equation for the reaction of nitrogen oxide, NO, with chlorine, Cl2, is:
2NO + Cl2 --> 2 NOCl</p>
<p>The initial rates of reaction for various concentrations of the reactants were measured and recorded at constant temperature as follows:</p>
<p>Experimental---<a href="M">NO</a>----<a href="M">Cl2</a>----DELTA [Cl2]/DELTA t (M/hr)
1--------------.25---------.50-----------.75
2--------------.25---------1.00----------3.02
3--------------.50---------2.00----------24.10</p>
<p>calculate the numerical value for the rate constant and specify the units</p>
<p>what is the order of this reaction with respect to each reactant and what is the overall order of the reaction</p>
<p>what is the rate of disappearance of Cl2 when the initial concentrations of the reactants are [NO]=.50M and [Cl2]=.10M</p>
<p>when Cl2 is disappearing at 4.5 M/hr, what is the rate of appearance of NOCl</p>
<p>what is the rate of appearance of NOCl when the initial concentrations of the reactants are: [NO]=.20M and [Cl2]=.30M</p>
<p>Can someone PLEASE help me figure out the steps involved to answer these questions?</p>