The reaction below was observed in a 4.0 L flask at 445 oC. H2 (g) +...
The reaction below was observed in a 4.0 L flask at 445 oC.
H2 (g) + I2 (g) ↔ 2 HI (g)
Initially, 0.20 atm of each gas (H2, I2 and HI) was placed in the flask. If the kp = 50.2 atm at 445oC, what is the equilibrium pressure (in atm) of HI (g)?
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The reaction below was observed in a 4.0 L flask at 445 oC.
H2 (g) +...
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.
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?
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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) = .
The reaction H2(g) + I2(g) <=> 2HI(g) has Kc = 50.2 at 718K. If a flask...
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Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and...
Suppose that 0.1000 mole each of H2 and I2 are placed in 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2 is found to be 0.0210 M. a) What are the equilibrium concentrations of H2 and HI, respectively? Calculate Kc for the following reaction at 425oC. H2(g) + I2(g) ⇄ 2 HI(g) b) If the initial concentrations of H2 and I2 are 1.000 M each, and the initial concentration of HI is 0.000,...
Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.69 −L flask at 500 K initially...
Consider the reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.69 −L flask at 500 K initially contains 0.377 g H2 and 17.93 g I2. At equilibrium, the flask contains 17.72 g HI. Calculate the equilibrium constant at this temperature.
The equilibrium constant for the following reaction is 50.5 at 448 oC. H2(g) + ...
The equilibrium constant for the following reaction is 50.5 at 448 oC. H2(g) + I2(g) ⇌ 2 HI(g) a. Find DGorxn at 448 oC. (This is the change in free energy when the partial pressure of each gas is 1 atm and the T is 448 oC.) b. What is DGrxn when T = 448 oC and PH2 = 1 atm, PI2 = 0.1 atm, PHI = 0.1 atm? c. Is the forward reaction spontaneous...
Given the reaction below, H2 (g)+ I2 (g)⇌ 2 HI (g) Kc = 50.5 What was...
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?
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.70 L flask at a certain...
Consider the following reaction: H2(g)+I2(g)⇌2HI(g) A reaction mixture in a 3.70 L flask at a certain temperature initially contains 0.766 g H2 and 97.0 g I2 At equilibrium, the flask contains 90.2 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. I keep getting 700 as the answer but it's not right.
H2(g)+I2(g)=2HI(g) The value of Kp for the reaction is 61.0 at 905 °C. What is the...
H2(g)+I2(g)=2HI(g) The value of Kp for the reaction is 61.0 at 905 °C. What is the equilibrium partial pressure of HI in a sealed reaction vessel at 905 °C if the initial partial pressures of H2 and I2 are both 0.260 atm and initially there is no HI present?
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,...
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