QQuestionChemistry
QuestionChemistry
The molar mass of LiF is 25.94 g/mol. How many moles of LiF are present in 10.37 g?
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Answer
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Step 1:I'll solve this problem step by step using the precise LaTeX formatting guidelines you specified:
Step 2:: Identify the Given Information
- Mass of LiF = $$10.37 \mathrm{~g}
- Molar mass of LiF = 25.94 \frac{\mathrm{g}}{\mathrm{mol}}
Step 3:: Set Up the Mole Conversion Formula
\text{Moles} = \frac{\text{Given Mass}}{\text{Molar Mass}}
To calculate moles, we use the formula:
Step 4:: Plug in the Values and Calculate
\text{Moles of LiF} = \frac{10.37 \mathrm{~g}}{25.94 \frac{\mathrm{g}}{\mathrm{mol}}}
Step 5:: Perform the Calculation
\text{Moles of LiF} = 0.400 \mathrm{~mol}
Final Answer
0.400 \mathrm{~mol} of LiF are present in 10.37 \mathrm{~g}.
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