C7H12 reacts with O2 to produce CO2 and H2O. Suppose 348 g of CO2 are produced in this reaction. What mass of O2 reacted?
398 g
In mass terms, the process requires 11 moles of oxygen (11 x 32 g = 352 g) to produce 7 moles of carbon dioxide (7 x 44 g = 308 g) of carbon dioxide.
In order to generate 348 g of carbon dioxide, we will require,
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To determine the mass of ( \text{O}_2 ) reacted, you can use stoichiometry. First, calculate the moles of ( \text{CO}_2 ) produced using its molar mass. Then, use the mole ratio between ( \text{CO}_2 ) and ( \text{O}_2 ) from the balanced chemical equation to find the moles of ( \text{O}_2 ). Finally, convert moles of ( \text{O}_2 ) to grams using its molar mass.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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