Chapter 15, Problem 76c
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(π) β 2 NO(π) + Br2(π) An equilibrium mixture in a 5.00-L vessel at 100Β°C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br2. (c) What was the mass of the original sample of NOBr?
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When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(π) β SO2(π) + Cl2(π) (a) Calculate πΎπ for this reaction at this temperature.
When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2: SO2Cl2(π) β SO2(π) + Cl2(π) (c) According to Le ChΓ’telier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?
A sample of nitrosyl bromide (NOBr) decomposes according to the equation 2 NOBr(π) β 2 NO(π) + Br2(π) An equilibrium mixture in a 5.00-L vessel at 100Β°C contains 3.22 g of NOBr, 3.08 g of NO, and 4.19 g of Br2. (b) What is the total pressure exerted by the mixture of gases?
Consider the hypothetical reaction A(π) β 2 B(π). A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0Β°C. At equilibrium, the partial pressure of A is 0.36 atm. (c) What could we do to maximize the yield of B?
As shown in Table 15.2, the equilibrium constant for the reaction N2(π) + 3 H2(π) β 2 NH3(π) is πΎπ = 4.34Γ10β3 at 300Β°C. Pure NH3 is placed in a 1.00-L flask and allowed to reach equilibrium at this temperature. There are 1.05 g NH3 in the equilibrium mixture. (b) What was the initial mass of ammonia placed in the vessel?
For the equilibrium PH3BCl3(π ) β PH3(π) + BCl3(π) πΎπ = 0.052 at 60 Β°C. (b) After 3.00 g of solid PH3BCl3 is added to a closed 1.500-L vessel at 60 Β°C, the vessel is charged with 0.0500 g of BCl3(π). What is the equilibrium concentration of PH3?