B. Temperature effects on reaction rates 1. Results 1average 2 3" 4 time (sec) 41.8 24.2 11.7 89.4 1/time (sec-¹) 0.046 0.0413 0.0855 0.0112 In(time) 3.379 3.186 2.459 4.493 Temp (°C) 29.5 35 40.8 12.8 Temp (K) 302.68 308.15 313.95 285.95 1/Temp (1/K) 0.003309 0.003245 0.003185 0.003497 2. Answer these questions: a. Show mathematically that a plot of In(time) versus 1/Temp should give a straight line with a slope of E/R. b. Graph In(time) vs. 1/Temp and determine the slope. From the slope calculate the activation energy of the reaction. 1/Temp 0.00355 0.0035 0.00345 0.0034 0.00335 0.0033 0.00325 0.0032 0.00315 Chart Title y = 0.0002x + 0.0028 R² = 0.9686 0.0031 0 1 N In (Time) E 4 5 3. Answer these questions: a. From the graph, determine the reaction time at 20 °C and 30 °C. b. For this particular reaction, how good is the rule of thumb that "a 10 °C increase should double the reaction rate"? Explain your answer.

Help with the questions like the objectives and the hypothesis and all of those

KINETICS AND EQUILIBRIUM Using Le Chatelier's Principle to predict the result of changing... Methane and water react to form hydrogen and carbon monoxide, like this: CH_(g)+H,O(g) …+ 3H,(g)+CO(g) perturbation The reaction is endothermic. Suppose a mixture of CH4, H₂O, H₂ and CO has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. change in composition The temperature is raised. The pressure of CO will ? The temperature is lowered. The pressure of CH4 will? ? go up. go down. not change. shift in equilibrium to the right to the left O (none) to the right to the left O (none) X 0/5 G

FOR THE REACTION CH4 (G) + 2 O2 (G) <- -> CO2 (G) + 2 H2O (L)  SHOW W ARROW HOW TO REDUCE THE FOLLOWING STRESSES TO THE REACTION (A) DECREASE THE TOTAL VOLUME OF THE SYSTEM (B) ADDITIONAL O2(G) IS ADDED TO THE SYSTEM

Hi! Can someone answer Learning Task 1? Explain the required answers briefly. Thanks !

1 10:44 7.5 student.pdf Approximation Kule: When can it be made? An approximation may be made when the initial concentration of the reactants is more than 1000x greater than the Keq. When this is the case, the change in the concentration of the reactants will be negligible at equilibrium. Thus the initial concentrations of the reactants can be used to represent the equilibrium centration of the reactants: i.e. [initial] reactants= [eq] reactants Sample Problem The atmosphere contains large amounts of nitrogen and oxygen gases which do not react under ordinary conditions. However, they do react under extreme conditions such as those produced by a flash of lightning or inside the running of a car engine. The production of nitrogen oxides from these exhaust gases are a huge pollution problem. If a chemist puts 0.085 mol of nitrogen and 0.038 mol of oxygen gas in a rigid 1.5 L cylinder. What is the concentration of nitrogen monoxide gas NO (g) in the mixture at equilibrium? N2 (9) + O2( 2…

This is no help to me because it is not an explanasion USING the collision theory

Calc solubility 2

Lequel des composés ci-dessous pourrait être utilisé comme réactif de départ dans la réaction suivante?

7) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3D