A student obtained the following data for the gas phase decomposition of phosphine at 120 °C. PH₂(g) →→→→1/4 P4(g) + 3/2 H₂(g) [PH3], M 9.40x10-2 time, s 0 4.70x10-² 29.9 2.35x10-2 59.8 1.18x10-2 89.7 (1) What is the half-life for the reaction starting at t = 0 s? What is the half-life for the reaction starting at t = 29.9 s? | Does the half-life increase, decrease or remain constant as the reaction proceeds? [ (2) Is the reaction zero, first, or second order? [ (3) Based on these data, what is the rate constant for the reaction?

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The following sequence of steps has been proposed for the overall reaction between H2 and Br2 to form HBr:(1) Br2(g) 2Br(g)Write the overall balanced equation and show that the overall Qc is the product of the Qc’s for the individualsteps.

I need help with this questions and show the work step by step?

Consider the following reaction where Kc = 5.10×10-6 at 548 K.NH4Cl(s) NH3(g) + HCl(g)A reaction mixture was found to contain 5.10×10-2 moles of NH4Cl(s), 3.00×10-3 moles of NH3(g), and 2.26×10-3 moles of HCl(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionA. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.

Methane and water react to form hydrogen and carbon monoxide, like this: CH₁(9)+H₂O(g) → 3H2(g)+CO(g) The reaction is endothermic. Suppose a mixture of CH 4, 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. perturbation change in composition shift in equilibrium to the right to the left The temperature is raised. The pressure of CH4 will ? ○ (none) to the right to the left The temperature is lowered. The pressure of CO will ? O (none) ×

⠀⠀ M Apple Google Disney ESPN Yahoo! Consider the reaction CO(g) + Cl₂(g) →→→COCI₂(g) ANSWER: Submit Answer kJ/mol Biomedical Careers Program Apple iCloud ☆ B prod03-cnow-owl.cengagenow.com Try Another Version Yahoo G G D2L Images Bing Google Wikipedia Facebook Twitter LinkedIn The Weather Channel Yelp TripAdvisor ☆ C S b b C G 凶 Using the standard thermodynamic data in the tables linked above, calculate AGxn for this reaction at 298.15K if the pressure of each gas is 10.91 mm Hg. D2L 1 item attempt remaining COWLv2 |... [References] Use the References to access important values if needed for this question. C + 88 M

8. Sketch an Energy Level Diagram with activation energy (Ea) OR a Maxwell-Boltzmann distribution. Use it to explain how the addition of a catalyst increases the rate of a reaction. (C: 4)

Gas Initial Concentration (M) H2 0.030 I2 0.015 HI ? Samples of three gases, H2(g) , I2(g) , and HI(g) , were combined in a rigid vessel. The initial concentrations of H2(g) and I2(g) are given in the table above. (a) The original value of the reaction quotient, Qc , for the reaction of H2(g) and I2(g) to form HI(g) (before any reactions take place and before equilibrium is established), was 5.56 . On the following graph, plot the points representing the initial concentrations of all three gases. Label each point with the formula of the gas.   Equilibrium was established at a certain temperature according to the following chemical equation. H2(g)+I2(g)⇄2HI(g)ΔH°rxn=−9.4kJ/molrxn;Kc=49 After equilibrium was established, the concentration of H2(g) was 0.020M . (b) On the graph above, carefully draw three curves, one for each of the three gases, starting from the initial points you drew in part ( a ). The curves must show how the concentration of each of the three gases changed…

I get using the Arrhenius equation but even after calculating the e-[82.64 KJ/mol)/(8.314 J/mol.K × 346.63 K)] it doesn't equal up to 3.518× 10-13 s-1. Where did it come from if it didn't from from just that?