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.
A sample of IBr decomposes according to the following equation: 2 IBr(g) 1 I2(g) + 1...
please help! A sample of So, decomposes according to the following equation: 2 503(g) = 2 50_1911040 An equilibrium mature in a 2-L vessel at 604 °C, contains 0.00928 g of So, 0.0150 gʻof So, and 0.00335 g of - (a) Calculate Kfor this reaction at this temperature. (b) What is the total pressure exerted by the equilibrium mature of gases? atm
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) = .
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?
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 reaction I2(g) + Br2(g) ⇌ 2 IBr(g) A vessel initially contains 2.50 M I2 and 2.50 M Br2. Determine the equilibrium concentration of IBr if KC for the reaction at this temperature is 3.27.
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 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...
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) =
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?
Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2 NF3(g) N2(g) + 3 F2(g) When 2.82 mol of NF3 is placed in a 2.50-L container and allowed to come to equilibrium at 800 K, the mixture is found to contain 0.0297 mol of N2. What is the value of Kp at this temperature? (R = 0.082057 L ⋅ atm/mol ⋅ K) a. 1.83 × 10–3 b. 4.43 × 10–7 c. 1.91 × 10–3 d....