Can you please write the experimental question below using the results provided on the table Chemical Kinetics 2: Temperature of the reaction: Oxalic acid - potassium permanganate reaction system experiment The reaction rate for the oxidation - reduction between oxalic acid, H2C204 and potassium permanganate, KMnO4, is measured by recording the time elapsed for the purple colour of the permanganate ion, MnO4 to disappear in the reaction: 5H2C2O 4 (aq) + 2KMnO4 (aq) + 3H2SO4 (aq) -> 10CO2 (g) + 2MnSO4 (ag) + K2SO2 (ag) + 8H2O (1) The rate of discharge of the purple colour of MnO4, can thus be used as a measure of the rate of the reaction. Results Experiment Number| Temperature,T ( c) | Time, t (s)| Log t-1 (s-1) (T+273) -1 (K-1) 1|30| 190,21 0,43| 3,30 x 10-3 21 40 58,01 0,571 3, 19 x 10-3 3| 50| 22,91 0,761 3,096 x 10-34|60| 13,0 | 0,891 3,003 x 10-3 5 70| 10,65 0,971 2,91 x 10-3 Questions 2. Plot a graph of log t^ -1 versus (T+ 273)^-1 and draw the best straight line through the points. 3. If the rate of the reaction is k[MnO4] where k is the rate constant, what conclusion can be drawn about the order of the reaction with respect to the oxalate? 4. If the relationship between k and the absolute temperature (T+273)^-1 is log k/s^-1 = -0.0521 Ea (T+273)^-1/kJmol1 + constant, calculate the activation energy, Ea of the reaction from the graph taking k to be equal to t^ -15. Is the inorganic salt a catalyst or not Give reasons for your answer. 6. From your results, state the effect of increasing the temperature on the rate of the reaction and determine the factor by which the rate changes when the temperature changes by 10\deg C. Results and calculations Table \table[[\table[[Experiment], [number]], \table[[Temperature,], [T(c) 田 Results and calculations Table Experiment number 1 -23456 C C Temperature, Time, t(s) Logt (s1) T(C) (T+273) (k-1) 30 40 848828 190,2 0,43 3,30 x 10 58,0 0.57 3,19 x 103 50 22.9 0.76 3,096 x 103 60 13.0 0.89 3,003 x 10-3 70 10,65 0.97 2,91 x 10-3 21,46 0.75 3,096 x 10³

Complete the table of reactants and products below and identify the limiting reactant.

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species H20 4 H,PO4 HNO, (Choose one) NO2 7 OH (Choose one) HF (Choose one) ▼

6. The oxidation of methylhydrazine, N,H,CH,(1), by dinitrogen tetroxide, N,O,(1), was used for propulsion in the Space Shuttle orbiter. This reaction is represented by the equation 4 N,H,CH;(1) + 5 N,0,(1) → 12 H,O(g) + 9 N,(g) + 4 CO,(g) The enthalpy of formation for liquid methylhydrazine is +53 kJ/mol and the enthalpy of formation for liquid dinitrogen tetroxide is -20 kJ/mol. Calculate AH° for this reaction. KU A

Give the expression for the Ksp for the following CACO3(s) Ca*2 CO3 2 Ksp = %3D

d The standard enthalpy change for the following reaction is -602 kJ at 298 K. AH° = -602 kJ Mg(s) + 1/2O₂(g) → MgO(s) ΔΗ — What is the standard enthalpy change for the reaction at 298 K? 2 MgO(s) →→→2 Mg(s) + O₂(g) kj Submit Answer Retry Entire Group 9 more group attempts remaining

Given the following data:     2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l)    ΔG0= -6399 kJ     C(s) + O2(g) → CO2(g) ΔG0= -394 kJ     H2(g) + ½O2(g) → H2O(l) ΔG0= -237 kJ       Calculate the ΔG0rxn for the reaction      6 C(s) + 3 H2(g) → C6H6(l)

13, :№= daw anews N=H daw amous here :0: N=CO 가 72 Q:C=N: КО KCN, HCL KO KCN, HCL gali KⓇ that product