Given the following balanced reaction of hydrochloric acid and oxygen gas forming chlorine gas and water, how many grams of hydrochloric acid will be needed to form 335 grams of chlorine gas, assuming there is excess oxygen present? (To find the molar mass in the problem, use the periodic table and round the mass to the hundreds place for calculation.) 4HCl(aq) + O2 ---> 2Cl2(g) + 2H2O(l)

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Given the following balanced reaction of hydrochloric acid and oxygen gas forming chlorine gas and water, how many grams of hydrochloric acid will be needed to form 335 grams of chlorine gas, assuming there is excess oxygen present? (To find the molar mass in the problem, use the periodic table and round the mass to the hundreds place for calculation.) 4HCl(aq) + O2 ---> 2Cl2(g) + 2H2O(l)

Chemistry
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@Darkhawke first of all is that reaction balanced? and if so how do you know?
@Darkhawke Please carry on with photon. Answer him.
Yes, the equation is balanced. However, I am unsure of how to solve this question.

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Well, you can tell if it's balanced by checking if you have the same number of atoms in the product and result. Here, you'll see that both sides have 2 oxygen, 4 chlorine, and 4 hydrogen.
To answer your main question, you'll need to use molar mass and some basic stoichemistry to get your answer. I highly advise learning this skill yourself, as it will come in handy many times.

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