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Part II: Kinetics (Rates of Reaction) For the reaction, 2 HI (g) → H2 (g) +...
Given the reaction below, H2 (g)+ I2 (g)⇌ 2 HI (g) Kc = 50.5 What was the initial mass of HI (g) placed in a sealed 1.50 L flask which resulted in 0.025 mol of each of H2 (g) and I2 (g) being found in the flask at equilibrium?
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI, H2, and I2? We were unable to transcribe this imageAt 6 °C the equilibrium constant for the reaction: 2 HI(g) = H2(g) + 12(g) is Kp = 2.66e-11. If the initial pressure of HI is 0.00837 atm, what are the equilibrium partial pressures of HI,...
Given the equilibrium reaction: 2HI(g) H2(g) + I2(g) A sample mixture of HI, H2, and 12, at equilibrium, was found to have [H2]- 1.4 x 102 Mand [HI 4.0 x 102 M. If Keq 1.0 x 10, calculate the molar concentration of I2 in the equilibrium mixture, Enter your answer in the provided box. ]= м
In an experiment to study the formation of HI(g), H2(g) + I2(g) <=> 2 HI(g) At equilibrium, {H2} = 0.0325, {I2} = 0.0987 and {HI} = 0.085. Calculate the value of Kc. Give your answer to 3 decimal places.
The disproportionation of hydrogen iodide, 2HI(g)-->H2(g)+I2(g), is an example of first order kinetics. (i) Write the rate law for this reaction. (ii) what are the units of k, the rate constant? Show how you determined the units (iii) Prepare a plot (sketch) of the [HI] versus time.
1.Consider the reaction: H2(g) + I2(s) = 2 HI(g) If 10.87 g H2 is mixed with 17.01 g I2, calculate the theoretical yield (g) of HI produced by the reaction. 2.For this reaction, 4.68 g nitrogen gas reacts with 8.61 g oxygen gas. nitrogen (g) + oxygen (g) = nitrogen monoxide (g) What is the maximum mass of nitrogen monoxide that can be formed?What is the FORMULA for the limiting reagent?What mass of the excess reagent remains after the reaction...
The reaction H2(g) + I2(g) → 2 HI (g) is first order in both hydrogen and iodine. It is therefore referred to as second order overall. Its rate constant for the formation of HI (g) at 400 ◦C is 2.34 × 10−2 · lit · mol−1 · sec−1 and its activation energy is 150 KJ/mol. Use the rate law to estimate how long it takes to form 0.1 mole of HI(g) if I start by putting 2 moles of H2...
Consider the following reaction: 2 HI(g) H2(g) + I2(g) If 2.29 moles of HI, 0.309 moles of H2, and 0.363 moles of I2 are at equilibrium in a 17.8 L container at 774 K, the value of the equilibrium constant, Kp, is
The rate constant for the gaseous reaction H2(g) + I2(g) → 2HI(g) is 2.42 × 10−2/(M·s) at 400°C. Initially an equimolar sample of H2 and I2 is placed in a vessel at 400°C and the total pressure is 1690 mmHg. (a) What is the initial rate (M·min) of formation of HI? (__________) (b) What are the rate of formation of HI and the concentration of HI (in molarity) after 13.4 min? Rate of formation = (_______) (c) [HI] = (_______)...
1. The kinetics of the following reaction have been studied: N2 + 3 H2 → 2 NH3 The rate of of appearance of NH3 was measured as ∆[NH3]/∆t = 9.00 x 10-2 mol L-1 s-1 (a) What is the rate of the reaction in mol L-1 s-1? (b) What is ∆[N2]/∆t in mol L-1 s-1? (c) What is ∆[H2]/∆t in mol L-1 s-1? 2. The initial rate of the reaction of species A and B A + 2 B →...