Answer:
79.91 g
Explanation:
First we <u>calculate the number of moles of 125.00 grams of copper (II) sulfate pentahydrate </u>(CuSO₄·5H₂O), using<em> its molar mass</em>:
- Molar Mass of CuSO₄·5H₂O = (Molar Mass of CuSO₄) + 5*(Molar Mass of H₂O)
- Molar Mass of CuSO₄·5H₂O = 249.68 g/mol
- moles CuSO₄·5H₂O = 125.00 g ÷ 249.68 g/mol = 0.501 mol CuSO₄·5H₂O
In the reaction, CuSO₄·5H₂O turns into CuSO₄.
So now <u>we convert 0.501 moles of CuSO₄ (anhydrous copper (II) sulfate) into grams</u>, using the <em>molar mass of CuSO₄</em>:
- 0.501 mol CuSO₄ * 159.609 g/mol = 79.91 g CuSO₄
Answer:
balanced chemical equation is
2 SiO₂ + 3 C₂ = 2 SiC + 4 CO
<span><span>KaAcid</span><span><span>1.0 * 109</span>Hydrobromic acidHBr</span><span><span>1.3 * 106</span>Hydrochloric acidHCl</span><span><span>1.0 * 103</span>Sulfuric acid<span>H2SO4</span></span><span><span>2.4 * 101</span>Nitric acid<span>HNO<span>3</span></span></span></span>
