QQuestionChemistry
QuestionChemistry
What mass of PH^3 (molar mass = 34.03 g/mol) is produced when 7.52 g of hydrogen reacts with excess phosphorus? (note: this is a special case where phosphorus exists as P^2
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Answer
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Step 1:: Write the balanced chemical equation for the reaction between hydrogen and phosphorus to produce phosphine (PH3).
The balanced equation is: P\_2 + 6H\_2 o 2PH\_3
Step 2:: Convert the given mass of hydrogen to moles using its molar mass.
The molar mass of hydrogen (H2) is 2 g/mol. The given mass of hydrogen is 7.52 g. To find the number of moles, divide the mass by the molar mass:
Step 3:: Determine the amount of phosphine (PH3) produced by stoichiometrically relating the moles of hydrogen.
From the balanced equation, we see that 6 moles of H^2 react with 1 mole of P^2 to produce 2 moles of PH^3. Since we have 3.76 moles of H^2, we can find the moles of PH^3 produced using cross-multiplication:
Step 4:: Convert the moles of phosphine to mass using its molar mass.
The molar mass of PH^3 is 34.03 g/mol. The moles of PH^3 are 1.2533 mol. To find the mass, multiply the moles by the molar mass: \text{Mass of } PH\_3 = \text{Moles of } PH\_3 \times \text{Molar mass of } PH\_3 \text{Mass of } PH\_3 = 1.2533 \text{ mol} \times 34.03 \text{ g/mol}
Final Answer
The mass of PH^3 produced is approximately 42.61 g.
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