2 Factors affecting the rate of a reaction.ConcentrationRatelaw速率方程ArrheniusEquation阿累尼乌斯方程式.Temperature·Catalysts.The physical state of the reactants
11 2 Factors affecting the rate of a reaction •Concentration ——Rate law 速率方程 •Temperature —— Arrhenius Equation阿累尼乌斯方程式 •Catalysts •The physical state of the reactants
2-1 Concentration白磷在纯氧气中燃烧白磷在含20%的氧气中燃烧The relationship between the rate and the concentrations oflaw for the reaction. It isreactants is called the ratedeterminedfrom the experimentaldata.初始速率法12
12 2-1 Concentration 白磷在纯氧气中燃烧 白磷在含20%的氧气中燃烧 The relationship between the rate and the concentrations of reactants is called the rate law for the reaction. It is determined from the experimental data.——初始速率法
Example 7-2 400C, CO (g) + NO, (g) =CO, (g) + NO (g)No.[CO] ini.[NO,lini.ro(mol/L)(mol/L)(mol·L-1.s-')10.100.100.00520.200.100.01030.300.100.01540.200.100.01050.100.300.015r α[CO][NO2]初始速率法13r = k[CO][NO,] = 0.5[COI[NO,]
13 Example 7-2 400℃, CO (g) + NO2 (g) = CO2 (g) + NO (g) No. [CO] ini. (mol/L) [NO2 ]ini. (mol/L) r0 (mol·L-1·s-1 ) 1 0.10 0.10 0.005 2 0.20 0.10 0.010 3 0.30 0.10 0.015 4 0.10 0.20 0.010 5 0.10 0.30 0.015 r ∝[CO][NO2 ] r = k[CO][NO2 ] = 0.5[CO][NO2 ] 初始速率法
Example7-3 800℃ , 2H2 + 2 NO = 2 H,O + N2No.rn2 (mol·L-1.s-l)[NO] (mol/L)[H] (mol/L)16.00× 10-31.00× 10-33.19× 10-326.00× 10-32.00×10-36.36x 10-336.00× 10-33.00×10-39.56x 10-341.00× 10-36.00× 10-30.48× 10-352.00×10-36.00× 10-31.92× 10-366.00× 10-34.30×10-33.00×10-3r α[H,][NO]2r = k [H,J[NO]2 = 8.86 × 104[H,I|NO]214
14 Example7-3 800℃ , 2H2 + 2 NO = 2 H2O + N2 No. [NO] (mol/L) [H2 ] (mol/L) rN2 (mol·L-1·s-1 ) 1 6.00 10-3 1.00 10-3 3.19 10-3 2 6.00 10-3 2.00 10-3 6.36 10-3 3 6.00 10-3 3.00 10-3 9.56 10-3 4 1.00 10-3 6.00 10-3 0.48 10-3 5 2.00 10-3 6.00 10-3 1.92 10-3 6 3.00 10-3 6.00 10-3 4.30 10-3 r ∝[H2 ][NO]2 r = k [H2 ][NO]2 = 8.86 104 [H2 ][NO]2
aA+bB+→gG+hHrate = k[A] α[B]βα is called the order ofA and β the order of B; α+β= n, n is calledreaction order (the sum of exponents in the rate equation)kis called rate constant for the reaction. The unit ofk is determined by the reaction order n.(mol-L-")l-n.s-1 or (mol-dm-3)1-n.s-1Unit:15
15 a A + b B + → g G + h H rate = k[A] [B] is called the order of A and the order of B; + = n , n is called reaction order ( the sum of exponents in the rate equation). k is called rate constant for the reaction. The unit of k is determined by the reaction order n. Unit：(mol·L-1 ) 1-n·s-1 or (mol·dm-3 ) 1-n·s-1