2N2O5(g)----> 4NO2(g) + O2(g)
<span>[N2O5]i (M) Initial Rate(M^-1 s^-1) </span>
<span>0.093 4.84x10^-4 ---- (1) </span>
<span>0.186 9.67x10^-4 ----- (2) </span>
<span>0.279 1.45x10^-3 ----- (3) </span>
<span>From equation (1) & (2) it is evident that when [N2O5}i is doubled the initial rate is doubled, which implies the rate is directly proportional to [N2O5]. Similarly comparing equation (1) & (3) we observe that when [N2O5] is tripled the rate is also tripled. Hence the rate equation is </span>
<span>Rate = k [N2O5] </span>
<span>Using the data of any equation, say (1), we get </span>
<span>4.84x10^-4 = k x 0.093 </span>
<span>OR k = 4.84x10^-4/0.093 = 5.2 x 10^-3 s-1 </span>
<span>Hence the rate law is </span>
<span>Rate = 5.2 x 10^-3 s-1[N2O5]</span>
CuSO4. 5H2O(s) → CuSO4(s) + 5 H2O(g)
Here, when we heat copper (II) sulphate pentahydrate, it will turn white in colour from blue colour.
Answer:
a. Oxidized: Fe(s)
Reduced: Pb(NO3)2
b.Oxidized: Cu(s)
Reduced: AgNO3
c. Oxidized: Al(s)
Reduced: AgNO3
Explanation:
In a redox reaction, one reactant is been oxidized whereas the other is reduced.. The reduced reactant is the one that is gaining electrons and the oxidized one is loosing electrons.
In the reactions:
a. 2Fe(s)+3Pb(NO3)2(aq)→3Pb(s)+2Fe(NO3)3(aq)
The Fe is as reactant as Fe(s) (Oxidation state 0) and the product is +3 (Because NO3, nitrate ion, is always -1). That means Fe is oxidized. The Pb as reactant is +2 and as product 0 (Gaining 2 electrons). Pb(NO3)2 is reduced
b. 2AgNO3(aq)+Cu(s)→2Ag(s)+Cu(NO3)2(a)
AgNO3 is +1 and Ag(s) is 0. AgNO3 is reduced. Cu(s) is 0 as reactant and +2 as product. Cu(s) is been oxidized
c. 3AgNO3(aq)+Al(s)→3Ag(s)+Al(NO3)3(aq)
Here, in the same way, AgNO3 is +1 as reactant and 0 as product. AgNO3 is reduced. And Al(s) is 0 as reactant but + 3 as product. Al(s) is oxidized.
Answer:
A.moles of solute per liter of solution
Explanation:
the total number of moles of substances present; mass percentage, the ratio of the mass of the solute to the mass of the solution times 100; parts per thousand (ppt), grams.
:-befrank
Answer: Option C - Radical
Explanation:
A radical is a chemical specie carrying a lone electron. In the halogenation of alkanes: take Methane CH4 as the alkane, and Chlorine Cl as the halogen.
The step by step halogenation process is as follows:
CH4 + Cl2 --> CH3• + HCl + Cl•
CH3• + Cl2 --> CH3Cl + HCl
CH3Cl + Cl2 --> CH2Cl2 + HCl + Cl•
CH2Cl2 + Cl2 --> CHCl3 + HCl
CHCl3 + Cl2 --> CCl4 + HCl + Cl•
Chlorine molecule attack methane knocking off an hydrogen atom from it and forming a methyl radical (CH3•), that is subsequently attack by another chlorine molecule. This cycle repeats itself, until no hydrogen atom is available for substitution by the highly reactive chlorine radical.
Note: no cation or anion is formed in the halogenation process