A sample of ascorbic acid (vitamin C) is synthesized in
the labor...

Question

A sample of ascorbic acid (vitamin C) is synthesized in
the laboratory. It contains 1.50 g of carbon and 2.00 g of
oxygen. Another sample of ascorbic acid isolated from
citrus fruits contains 6.35 g of carbon. According to the
law of constant composition, how many grams of oxygen
does it contain?

Accepted Answer

Hey everyone in this example, we have a sample of acetic acid composed of 2.05 g of carbon and 2.73 g of. We need to calculate the mass of carbon in another sample of acetic acid Of 3.27 g of oxygen. And so what this second part of this question is describing to us is finding our mass ratio of oxygen to cart. And so what we're going to take is our ratio of oxygen to carbon. So according to the prompt, we have 2.73g of oxygen Divided by our ratio of carbon, which is given in the prompt as 2.05 g of carbon. And this gives us a ratio or a mass ratio equal to 1.33 2, 1 Atom of carp. And so because we know that this is our ratio of oxygen to carbon, we're going to go ahead and interpret this based on our second mass given for oxygen, Which has given us 3.27 g of oxygen. So we're going to divide this by that given mass ratio of 1. grams of And so this is going to equal a value of 2.4 59 g of carbon. And so this will complete this example as our final answer. So if you have any questions, please leave them down below. Otherwise, I'll see everyone in the next this video

A sample of ascorbic acid (vitamin C) is synthesized in the laboratory. It contains 1.50 g of carbon and 2.00 g of oxygen. Another sample of ascorbic acid isolated from citrus fruits contains 6.35 g of carbon. According to the law of constant composition, how many grams of oxygen does it contain?

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