Question
A sample of a hydrocarbon contains 2075 g C and 4.25 g H. Its molar mass is 58.04g/mol What is its empirical formula C_(2)H_(5) is CH_(2) is CH C_(5)H COMPLETE What is its molecular formula? Type in the correct number based on the label C_(A)H_(B) A: square B: square DONE V
Answer
4.2
(295 Votes)
Ollie
Professional · Tutor for 6 years
Answer
The empirical formula is
.The molecular formula does not fit the provided options as it results in fractional values, suggesting a need to re-evaluate the initial data or assumptions.
Explanation
## Step 1: Determine the moles of carbon and hydrogen in the sample.### **
**### **
**## Step 2: Determine the simplest ratio of moles of C to H.### **\(\text{ratio of C} = \frac{\text{moles of C}}{\min(\text{moles of C}, \text{moles of H})} = \frac{172.68}{4.21} \approx 41\)**### **\(\text{ratio of H} = \frac{\text{moles of H}}{\min(\text{moles of C}, \text{moles of H})} = \frac{4.21}{4.21} \approx 1\)**## Step 3: Form the empirical formula based on the ratio.### **
**## Step 4: Calculate the molar mass of the empirical formula.### **
**## Step 5: Determine the number of empirical formula units in the molecular formula.### **
**## Step 6: Form the molecular formula.### **
**#