10.5 milliliters of 3.5 M zinc hydroxide react completely with 15.0 milliliters of 4.9 M nitric acid.
<h3>What is molarity?</h3>
It is a unit of concentration equivalent to moles of solute per liter of solution.
- Step 1: Write the balanced equation.
Zn(OH)₂ + 2 HNO₃ ⇒ Zn(NO₃)₂ + 2 H₂O
- Step 2: Calculate the reacting moles of Zn(OH)₂.
10.5 mL of 3.5 M Zn(OH)₂ react.
0.0105 L × 3.5 mol/L = 0.037 mol
- Step 3: Calculate the reacting moles of HNO₃.
The molar ratio of Zn(OH)₂ to HNO₃ is 1:2.
0.037 mol Zn(OH)₂ × 2 mol HNO₃/1 mol Zn(OH)₂ = 0.074 mol HNO₃
- Step 4: Calculate the molarity of HNO₃.
[HNO₃] = 0.074 mol / 0.0150 L = 4.9 M
10.5 milliliters of 3.5 M zinc hydroxide react completely with 15.0 milliliters of 4.9 M nitric acid.
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This law states that, despite chemical reactions or physical transformations, mass is conserved — that is, it cannot be created or destroyed — within an isolated system. In other words, in a chemical reaction, the mass of the products will always be equal to the mass of the reactants.
I looked this up but hope it helps!
Answer:
166 g
Explanation:
Step 1: Write the reaction for the obtaining of Fe from magnetite
Fe₃O₄ ⇒ 3 Fe + 2 O₂
Step 2: Calculate the moles corresponding to 120 g of Fe
The molar mass of Fe is 55.85 g/mol.
120 g × (1 mol/55.85 g) = 2.15 mol
Step 3: Calculate the moles of Fe₃O₄ required to produce 2.15 moles of Fe
The molar ratio of Fe₃O₄ to Fe is 1:3. The moles of Fe₃O₄ required are 1/3 × 2.15 mol = 0.717 mol
Step 4: Calculate the mass corresponding to 0.717 moles of Fe₃O₄
The molar mass of Fe₃O₄ is 231.53 g/mol.
0.717 mol × 231.53 g/mol = 166 g
Answer:
The answer is given below in the picture
Explanation:please check it
