(g)+Cl2(g)⇌2BrCl(g) @ 400K, Kc=7.0 Part A: If 0.54 mol of Br2 & 1.23 mol of Cl2Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units. Part B: If 0.54 mol of Br2 & 1.23 mol of Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units.
For the equilibrium: Br2(g)+Cl2(g)⇌2BrCl(g) @ 400K, Kc=7.0
Part A: If 0.54 mol of Br2 & 1.23 mol of Cl2Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Br2? Express your answer to two significant figures and include the appropriate units.
Part B: If 0.54 mol of Br2 & 1.23 mol of Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of Cl2? Express your answer to two significant figures and include the appropriate units.
Part C: If 0.54 mol of Br2 & 1.23 mol of Cl2 are introduced into a 3.0-L container @ 400K, what will be the equilibrium concentration of BrCl? Express your answer to two significant figures and include the appropriate units.
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