# When 1.50 g of copper is heated in air, it reacts with oxygen to achieve a final mass of 2.14 g. How do you calculate the empirical formula of this copper oxide?

See below.

Recall that by using the molar mass of an element and the mass of the element in the sample, you can find the amount of moles in the sample. We're gonna find the moles of copper and oxygen within the sample of copper oxide.

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Determine the mass of oxygen by subtracting the initial mass of copper from the final mass of copper oxide. Convert the masses to moles. Find the mole ratio by dividing each mole value by the smallest mole value. If necessary, multiply to obtain whole numbers. The resulting ratio represents the empirical formula.

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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.

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