Chemistry: Molecular Approach (4th Edition)

Published by Pearson
ISBN 10: 0134112830
ISBN 13: 978-0-13411-283-1

Chapter 4 - Exercises - Page 191: 115


6.9 g

Work Step by Step

1. There are two reactions in this process: $$2Ba(s) + O_2(g) \longrightarrow 2 BaO(s)$$ $$BaO(aq) + H_2O(l) \longrightarrow Ba^{2+}(aq) + 2 OH^-(aq)$$ 2. Calculate the amount of moles of $OH^-$: $$1.0 \space L \times \frac{0.10 \space mol \space OH^-}{1 \space L} = 0.10 \space mol \space OH^-$$ 3. Find the amount of moles of barium metal: $$0.10 \space mol \space OH^- \times \frac{1 \space mol \space BaO}{2 \space mol \space OH^-} \times \frac{2 \space mol \space Ba}{2 \space mol \space BaO} = 0.050 \space mol \space Ba$$ $ Ba $ : 137.3 g/mol - Using the molar mass as a conversion factor, find the mass in g: $$ 0.050 \space mole \times \frac{ 137.3 \space g}{1 \space mole} = 6.9 \space g$$
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