A mixture of 1.374 g of H_2 and 70.31 g of Br_2 is heated in a 2.00 L vessel at 700 K. These substances react as follows: H_2 (g) + Br_2 (g) 2 HBr (g) At equilibrium the vessel is found to contain 0.566 g of H_2. Calculate the equilibrium concentration of HBr. Express your answer using three significant figures. Use the following values in your calculations: molar mass of H_2 = 2.0159 g/mol and molar mass of Br_2 = 159.81 g/mol. Do not round any of your values in your calculations to the requested number of significant figures until the very last step.
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Home » Chemistry » A mixture of 1.374 g of H_2 and 70.31 g of Br_2 is heated in a 2.00 L vessel at 700 K. These substances react as follows: H_2 (g) + Br_2 (g) 2 HBr (g) At equilibrium the vessel is found to contain 0.566 g of H_2.