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Aneli [31]
2 years ago
5

I really can’t do this don’t understand it

Chemistry
1 answer:
masya89 [10]2 years ago
3 0

Answer:

7.96g, 33.79%

Explanation:

I'll try my best to explain the entire process behind this question ;)

From the question, you can write the reaction

2H_2O(l)->2H_2(g)+O_2(g)

Now, there are a few reasons it is like this. Oxygen is a diatomic element, meaning it doesn't and can't exist as just O. It exists as O₂. To balance, this, double the amount of water and hydrogen so there is an equal amount of  each element on both sides of the reaction (4 H's, 2 O's on the reactant side, and 4 H's, 2 O's on the product side).

From this we can get a mole-to-mole ratio.

Onto the stoichiometry. Our goal in this is to convert from grams of water to grams of hydrogen, and we do so with a mole to mole ratio.

71.0gH_2O*\frac{1molH_2O}{18.02g} *\frac{2molH_2}{2molH_2O}* \frac{2.02g}{1molH_2}\\\\ =7.96gH_2

Basically, what I did was divide by water's molar mass to get moles of water, multiplied by the mole-to-mole ratio (2:2) to get moles of H2, and then multiplied by H2's molar mass to get what should be the amount of H2 produced by the reaction.

For percent yield, you can calculate it is such:

\frac{Actual}{Theoretical}*100

Plug the numbers in:

\frac{2.69g}{7.96g}*100\\\\ =33.79%

So, the percent yield is 33.79%

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A sample of gas has a volume of 2.36 L at a temperature of 53.00 °C. The gas sample is heated to a temperature of 139.00 °C (ass
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Explanation:

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5 0
3 years ago
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