For the equilibrium |
Part A If 2.2×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? Express your answer to two significant figures and include the appropriate units.
SubmitMy AnswersGive Up Part B If 2.2×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? Express your answer to two significant figures and include the appropriate units.
SubmitMy AnswersGive Up Part C If 2.2×10?2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of Br2 after equilibrium is reached? |
For the equilibrium 2IBr(g)?I2(g)+Br2(g) Kp=8.5×10?3at 150 ?C. Part A If 2.2×10?2 atm of IBr is placed...
For the equilibrium 2IBr(g)⇌I2(g)+Br2(g) Kp=8.5×10−3 at 150 ∘C. a.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached? b.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached? c.)If 2.7×10−2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of Br2 after equilibrium is reached? a.)If 2.7×10−2 atm of IBr is...
For the equilibrium 2IBr(g) ⇌ I2:(g) + Br2(g) Kp = 8.5 x 10-3 at 150°C. Part A If 2.9x10-2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of IBr after equilibrium is reached?
For the equilibrium 2IBr(g) ⇌ I2:(g) + Br2(g) Kp = 8.5 x 10-3 at 150°C. Part B If 2.9x10-2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of I2 after equilibrium is reached?
IBr(g) is in equilibrium with I2(g) and Br2(g) at 150 ºC: 2 IBr(g) I2(g) + Br2(g) K = 8.50 x10^-3initially, a closed vessel at 150 ºC has a partial pressure of IBr of 0.350 atm and partial pressures of I2 and Br2 each of 0.750 atm. What is the partial pressure of IBr once the system reaches equilibrium?
At 1425 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 0.937. If the initial pressure of IBr is 0.00957 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = ____. p(I2) = _____. p(Br2) = _____ .
At 659 oC the equilibrium constant for the reaction: 2 IBr(g) I2(g) + Br2(g) is KP = 2.92. If the initial pressure of IBr is 0.00897 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = . p(I2) = . p(Br2) = .
Methane, CH4, reacts with I2 according to the reaction CH4(g)+I2(g)⇌CH3I(g)+HI(g) At 630 K, Kp for this reaction is 2.26×10−4. A reaction was set up at 630 K with initial partial pressures of methane of 105.1 torr and of 7.96 torr for I2. Part A Calculate the pressure, in torr, of CH4. Express your answer to four significant figures and include the appropriate units. SubmitMy AnswersGive Up Part B Calculate the pressure, in torr, of I2. Express your answer to three...
At 984 °C the equilibrium constant for the reaction: 2 IBr(g) = 12(g) + Br2(g) is Kp = 1.52. If the initial pressure of IBr is 0.00596 atm, what are the equilibrium partial pressures of IBr, I2, and Brz? P(IBr) = P(12) = p(Br2) =
1 Review Constants 1 Periodic Table For the equilibrium 21Br(9) = 1:(9) + Brz(9) K, -8.5 x 10- at 150°C. X Incorrect; Try Again; 5 attempts remaining Part If 2.9x10-2 atm of IBr is placed in a 2.0-L container, what is the partial pressure of Br, after equilibrium is reached? Express your answer to two significant figures and include the appropriate units. Value Units Submit Request Answer
A sample of IBr decomposes according to the following equation: 2 IBr(g) 1 I2(g) + 1 Br2(g) An equilibrium mixture in a 3-L vessel at 2695 oC, contains 0.0166 g of IBr, 0.0131 g of I2, and 0.0103 g of Br2. (a) Calculate KP for this reaction at this temperature. KP = . (b) What is the total pressure exerted by the equilibrium mixture of gases? Ptotal = atm.