1.
For the reaction below, the enthalpy of reaction isΔrH° = 29.36 kJ mol−1 and thethermodynamic equilibrium constant is K = 2.17 at 298.15K.
Cl2(g) + Br2(l) ⟶ 2 BrCl(g)
What is the value of K at 578 K ?
Enter your answer with 3 significant figures.Enter 1.25×10−4 as 1.25e−4 and7.38×102 as 7.38e2.
K = ____ at 578 K
2.
1 (58.1 KiB) Viewed 27 times
Suppose that A and B react to form C according to the equation below. A+2B=C What are the equilibrium concentrations of A, B and C if 2.8 mol A and 2.8 mol B are added to a 1.0 L flask? Assume that the equilibrium constant for this reaction is Kc = 5.1x10¹1. Hint: The equilibrium constant for this reaction is quite large. Therefore, the reaction goes almost 100% to completion. Enter your answers with two significant figures. Do not include units as part of your answer. -10 Use exponential notation (e.g. enter 1.2x10-¹ as 1.2e-10; enter 1.2x1015 as 1.2e15.) Equilibrium concentration of A: Number Equilibrium concentration of B: Number Equilibrium concentration of C: Number mol L -1 mol L-1 mol L-1
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