At t = 15 minutes has the reaction actually stopped? Explain your answer at the macroscopic level and the molecular level. Use the editor to format your answer
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- If Ch4=0.1M,O2=0.25M,CO2=0.35M and H2O=0.15 which direction will the reaction proceed.Enter your answer in the box provided. Consider the following reaction, which takes place in a single elementary step: 2A +B kf ⇌ kr A2B If the equilibrium constant Kc is 25.2 at a certain temperature and kr = 5.10 ×10−2 s, calculate the value of kf. ______ M−2s−14B(s) + 3O2(g) → 2B2O3(s) ∆HO= -2543.8 kJ Calculate the ∆HO for the decomposition of B2H6into its elements.
- 2a) explain the difference between the net energy change of a reaction and the activation energy of the same reaction40 The role of a catalyst is to change ______________. Select one: a. gibbs energy of reaction. b. enthalpy of reaction. c. activation energy of reaction. d. equilibrium constant.. Balance the following reaction and write the reaction rate ____CH3NH2(g) + ___O2 à ___CO2(g) + ___H2O(g) + ___N2(g)
- To determine the rate of the following reaction what physical property could be measured?H2 + I2 -> 2HI a) Change in concentration b) Change in pressurec)Change in colour d)Change in pH e) Change in massIn a hypothetical reaction of 2B + C ➡ D, the order of reaction for the given equation is??The oxidation of bromide ions is thought to occur by the following mechanism: H+ + H2O2 ↔ H2O+–OH (rapid equilibrium) H2O+–OH + Br– → HOBr + H2O (slow) HOBr + H+ + Br– → Br2 + H2O (fast) Which of the following statements is correct? A) The overall reaction equation is 2H+ + H2O2 + 2Br– → Br2 + H2O B) Rate = k[H2O2][H+][Br–] C) H+ is a catalyst. D) H2O is a reaction intermediate.
- Consider the reaction: 2N2 (g) + 5O2 (g) D 2N2O5 (g) + energy How will the concentration of N2 be affected, if there is a decrease in the concentration of N2O5?Consider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 d. What is the order of the reaction. e. Express the rate law and the integrated form equation. Is the reaction elementary? f. If the rate constant k = 1.61x10-5s-1 and [A0] = 4M, find the period of time between the 12th and 13th half-life. *g. If, for the same reaction, at the same temperature, we were to add a catalyst, would Ea, A, k and v be larger, smaller or equal? Explain.Consider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.