The temperature dependence of the rate constant for a re- action is tabulated as follows: Temperature (K) k (M-s-) 600 0.028 650 0.22 700 1.3 750 6.0 800 23 Calculate Eq and A.

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…

DWLV2 ohline pr calculater C3H70H(g) C2H6CO(g) H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 37 mL (d = 0.7 tps://cvg.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity isopropyl alcohol is placed in a 7.5 L vessel and heated to 180°C, what percentage remains undissocilated at equilibriu plus) [References] Isopropyl alcohol is the main ingredient in rubbing alcohol. It can decompose into acetone (the main ingredient in nail polish remover) and hydrogen gas according to the following reaction: C;H¬OH(g) = C,H,CO(g) + H2(g) At 180°C, the equilibrium constant for the decomposition is 0.45. If 43 mL (d= 0.785 g/mL) of isopropyl alcohol is placed in a 2.0L vessel and heated to 180°C, what percentage remains undissociated at equilibrium? %3D Submit Answer Try Another Version 3 item attempts remaining Previous Next 11:48 PM 73°F Partly sunny ^ 6/15/2021

A student was calculating k c for Trial 5. If the reaction follows Pathway 2 (formula below), what is the value of K if the initial concentration of Fe 3+ is 0.001000 M and the initial concentration of SCN - is 0.001000 M and the concentration of iron thiocyanate product is 9.694 x 10 -5 M.Fe 3+ (aq) + 2 SCN - (aq) → FeSCN 2 + (aq)