Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- Consider the reaction data. A⟶productsA⟶products ? (?)T (K) ? (?−1)k (s−1) 275275 0.3800.380 675675 0.7470.747 a)What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all value x1=? x2=? y1=? y2=? b)Determine the rise, run, and slope of the line formed by these points. c)What is the activation energy of this reaction?arrow_forwardThe study of the kinetics of the decomposition reaction of N205 gas was carried out in a closed cylinder with a volume of 1 L. The reactions that occur are: 2N2O5 (g) → 4N02(g) + O2(e) The following is a curve of 1/N205 against the reaction time of decomposition of N205 gas at temperatures of 427K and 527K. y = 2,0923x - 3,75 R² = 0,9999 0,7708x + 146,96 R² = 0,9995 ¥=0,7708x + 146,96 R² = 0,9995 %3D Time (sekon) a. Determine the rate equation for the decomposition reaction of gas N205 b. Determine the value of the rate constant (k) for the reaction at both temperatures. Express in the correct units. 1/[N,Og] (L/mol)arrow_forwardFor the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constantarrow_forward
- Q1arrow_forward3 / 3 100% + | 5. The following series of reactions show the catalyzed conversion of oxygen to ozone: ½ 0, (g) + NO (g) → NO, (g) 2 NO, (g) → NO (g) + O (g) 2 O, (g) + O (g) → 0, (g) -> a) Write the overall reaction. b) Is NO, or NO the catalyst for this reaction? Explain your answer. the following reaction:arrow_forwardConsider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of αarrow_forward
- 6b please!arrow_forward1) Use Hess's Law to determine AH for the following target reaction. 3 CO₂(g) + 4 H₂O(g) b) C3Hg(g) + 5 O₂(g) C(s) + O₂(g) -CO₂(g) 2 H₂(g) + O₂(g) 3 C(s) + 4 H₂(g) →→→ 2 H₂O(g) C3H8(g) AH = AH = ΔΗ ΔΗ = ??? -2043 kJ -393.5 kJ -483.6 kJarrow_forward8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.arrow_forward
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