When HI(g) is heated to 700 K, it reversibly decomposes to H2(g) and I2(g). The reaction...
When HI(g) is heated to 700 K, it reversibly decomposes to H2(g) and I2(g). The reaction is- 2 HI(g) ⇌ H2(g) + I2(g). A 15.00-L vessel at 700 K initially contains HI(g) at a pressure of 4.00 atm. When equilibrium is reached, it is found that the partial pressure of H2(g) is 0.387 atm. What is the partial pressure of HI(g) at equilibrium? A) 4.00 atm B) 3.61 atm C) 3.23 atm D) 4.39 atm E) 0.387 atm
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When HI(g) is heated to 700 K, it reversibly decomposes to H2(g)
and I2(g). The reaction...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g)...
The equilibrium constant, Kp, for the following reaction is 55.6 at 698 K: H2(g) + I2(g) 2HI(g) Calculate the equilibrium partial pressures of all species when H2 and I2, each at an intitial partial pressure of 1.65 atm, are introduced into an evacuated vessel at 698 K.
H2(g)+I2(g)⇌2HI(g) For the above reaction, Kc=55.3 at 700 K. In a 2.00-L flask containing an equilibrium...
H2(g)+I2(g)⇌2HI(g) For the above reaction, Kc=55.3 at 700 K. In a 2.00-L flask containing an equilibrium mixture of the three gases, there are 0.053 g of H2 and 4.39 g of I2. What is the mass of HI in the flask?
at 1000 K? for the reaction 12. The equilibrium constant, K 2 HI(g) H2(g) I2(g) is 55 at 425 C. Ifa 0.40 mol sample...
at 1000 K? for the reaction 12. The equilibrium constant, K 2 HI(g) H2(g) I2(g) is 55 at 425 C. Ifa 0.40 mol sample of HI was introduced into a 1.00 mL. reaction vessel at 425 C, what are the equibrium concentrations of H2, 12, and HI? 13. Consider the following reaction which is at equilibrium at 25 C 2 NH3(g) + CO2(g) A-152.2 kJ Ni4(NH2CO2X) In which direction will the reaction shift if (a) the pressure is increased (b)...
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K....
The equilibrium constant for the reaction: H2(g) + I2(g) <--> 2HI(g) is 54 at 700 K. A mixture of H2, I2 and HI, each at 0.020 M, was introduced into a container at 700 K. Which of the following is true? At equilibrium, [H2] = [I2] = [HI]. No net change occurs because the system is at equilibrium. The reaction proceeds to the left producing more H2(g) and I2(g). The reaction proceeds to the right producing more HI(g). At equilibrium,...
At 6 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP...
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,...
At 500°C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) +12(9) For HI(9) heated to...
At 500°C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) +12(9) For HI(9) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H, 1 = 0.383 M, L1=0.383 M, and [HI] = 3.24 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached?
At 49 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP...
At 49 oC the equilibrium constant for the reaction: 2 HI(g) H2(g) + I2(g) is KP = 4.83e-11. If the initial pressure of HI is 0.00862 atm, what are the equilibrium partial pressures of HI, H2, and I2? p(HI) = p(H2) = . p(I2) = .
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn= 55.3kJ At 298 K, a reaction vessel initially contains...
Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn= 55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage of N2O4 decomposes at 380 K ? Assume that the initial pressure of N2O4 is the same (0.100 atm).
Given the reaction at a certain temperature: H2(g) + I2(g) ↔ 2 HI(g). At equilibrium, the...
Given the reaction at a certain temperature: H2(g) + I2(g) ↔ 2 HI(g). At equilibrium, the partial pressure of HI is 3.8×10–3 atm and the partial pressures of H2 and I2 are 0.20 atm each. The Kp of this reaction is [X]. (Fill in the blank; report with correct number of significant figures.
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations...
Calculate the equilibrium concentrations of H2, I2, and HI at 700 K if the initial concentrations are [H2] = 0.200 M and [I2] = 0.400 M. The equilibrium constant Kc for the reaction following reaction is 57.0 at 700 K. (Show Work) H2(g)+I2(g)<--- ---->2HI(g)
at 1000 K? for the reaction 12. The equilibrium constant, K 2 HI(g) H2(g) I2(g) is 55 at 425 C. Ifa 0.40 mol sample of HI was introduced into a 1.00 mL. reaction vessel at 425 C, what are the equibrium concentrations of H2, 12, and HI? 13. Consider the following reaction which is at equilibrium at 25 C 2 NH3(g) + CO2(g) A-152.2 kJ Ni4(NH2CO2X) In which direction will the reaction shift if (a) the pressure is increased (b)...
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,...
At 500°C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) +12(9) For HI(9) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H, 1 = 0.383 M, L1=0.383 M, and [HI] = 3.24 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached?
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