Question

3. Experiments are done to study the reaction between aqueous chlorine dioxide and hydroxide ions: 2 CIO2 (aq) + 2 OH- (aq) → C103- (aq) + ClO2- (aq) + H20 (1) Exp. # Temp (°C) [CIO2), M [ОНН, М Initial rate, M/s 125 0.015 0.050 0.0026 25 0.045 0.050 0.0234 0.060 0.080 0.0665 4 35 0.060 0.040 0.1022 25

Answer 1

Guven- van 26 Trail 2 ca) Foot 2002 (aq) + 206”laq.) - 403.609.) + cios (89.) + Hedley Rate Law » Rate of reaction = K[C10,7*[04-14 [C102] = 0.015 M (T-050) [on-] = 0.05 m Rate of reachen = 0.0026 Mls putting the values in rate law. 0.0026 = K (0.015)(0.05)% -0 Traila (40.] =6.045 m (75251) 10. Conej = 0.05m Rate of reaction=0.0234 mis putting these values in rate law - 0.0234 = K (0.045)% (0.05)% - dividing eq© by eq Olen divid eq@ - 0.0234 = x (0.045)? Co-osty e90 0.0026 W (0.015) (0.0518 => 9 = 1 9 - (31% (3)= (3j2 x = 20 Trail 3 (402)=0.06 Con) a 0.08 Rate of reaction = 0.0665 M/S putting the values in rate laws - 0.0665 = k 10.069%0.0834

0.0026 dividing eq@ by eq o her 98 = 0.0665 K (0.06% (0.08) W 10.015)*10.0534 We have calculated x= 2 =) 25.576 = (0.06 ). ( 0.08 ) 3 d5:576 = (4)% 1395 § 25.57 31203 tot (1.67% 0. 0 3 ly = J

Traily (Te 35°C) [Clo, J-0.06M [ow-) = 0.04M Route of reaction = 0.1022 m/s Joi 0.1022 = Kze (0.06) (0.04) -@ from trail 3, 0.0665 : Kesec (0.06)? 10.08)". - 01022 - K35€ (0.0052 (0.04)! en 0.0665 kort lootge (0.03)" => 1.536 - Waste modelos Karc otropy 1536 = K352 * Kare (2 tamen gegen za 3 1536 x2 =k35c A re karc 2 3.633 - scºt od) 0 A = x Kasturi ainadrott K350 = 3-0736 keso = On increasing the s temperature, rare constant increases. Question 2. more cio, is dissolved in the solution - "! rate of reaction a [40] Son rate of reaction will increase

di dissolve more cing in the solution. Since rate of reaction is independent of concentration of clos" Joe rate of reachton remain the same 3. Add more Hoold) to the solution. org • Addition of water leads to dilution. So, on adding water, concentration of clog and OH will decrease . Thus, even though water is not present in rate laws, it will affect concentration of cing and onº, which participate in rate law. ? So, save of reaction will decrease 7. 4. As we have that, rate constant (K) is directly proportional to temperature, so on decreasing the temperature, rade constant, k will decrease and thes date of reachon we'll also decrease Also from Arrhenices equation, K = A exp.l-Eq) taking in 2) Ink: -Eq + In A negali ne po AT w negatiue positive So, Temp ↑ = lnka KA Of Temp. && tnkt aku № n dесrеліку вирелашле, kuwч фестиле).