Multiple Choice
Given 10.0 g of phosphorus (P) and 35.0 g of chlorine (Cl2), what mass of phosphorus pentachloride (PCl5) can be produced?
3. Chemical Reactions
Stoichiometry
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What volume of 0.242 M H2SO4 is needed to completely react with 56.8 mL of 0.120 M NaOH according to the equation H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)?
A
56.8 mL
B
7.05 mL
C
28.2 mL
D
14.1 mL
Verified step by step guidance1
Identify the balanced chemical equation: H2SO4(aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l). This tells us that 1 mole of H2SO4 reacts with 2 moles of NaOH.
Calculate the moles of NaOH using its concentration and volume. Use the formula: \( \text{moles of NaOH} = \text{concentration} \times \text{volume} \). Convert the volume from mL to L by dividing by 1000.
Determine the moles of H2SO4 needed using the stoichiometry from the balanced equation. Since 1 mole of H2SO4 reacts with 2 moles of NaOH, divide the moles of NaOH by 2 to find the moles of H2SO4 required.
Calculate the volume of H2SO4 needed using its concentration. Use the formula: \( \text{volume of H2SO4} = \frac{\text{moles of H2SO4}}{\text{concentration of H2SO4}} \).
Convert the volume of H2SO4 from liters to milliliters by multiplying by 1000 to find the final volume needed.
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