QQuestionChemistry
QuestionChemistry
Consider the compound Pb(SO4)2 and answer the following questions:
A. What is the name of this compound?
Lead (IV) Sulfate
B. What is the molar mass of this compound? Explain how you calculated this value.
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify the Chemical Formula
The chemical formula is $$\text{Pb(SO}_{4}\text{)}_{2}
Step 3:: Determine the Oxidation States
- Sulfate ($$\text{SO}_{4}^{2-}$$) has a standard oxidation state of -2
- Lead (Pb) has an oxidation state of + 4
Step 4:: Calculate the Molar Mass
\begin{aligned}
To calculate the molar mass, we'll add the atomic masses of each element: Lead (Pb): - Number of Pb atoms = 1 Sulfur (S): - Number of S atoms = 2 Oxygen (O): - Number of O atoms = 8 (4 × 2) Molar Mass Calculation: \text{Molar Mass} &= (1 \times 207.2) + (2 \times 32.07) + (8 \times 16.00) \ &= 207.2 + 64.14 + 128.00 \ &= 399.34 \text{ g/mol} \end{aligned}
Final Answer
A. Name: Lead (IV) Sulfate B. Molar Mass: 399.34 \text{ g/mol}
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