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Chemistry 99 Online
OpenStudy (anonymous):

Consider the equation. mc016-1.jpg Which represents the correct mass-volume relationship at STP? ~ 32.00 g of O2 react with an excess of H2 to produce (2 x 22.4) L of H2O. ~ 2.00 g of H2 react with an excess of O2 to produce (2 x 22.4) L of H2O. ~ 32.00 g of O2 react with an excess of H2 to produce 22.4 L of H2O. ~ (2 x 2.00) g of H2 react with an excess of O2 to produce 22.4 L of H2O.

OpenStudy (anonymous):

The picture is the jpg missing from the post.

OpenStudy (aaronq):

The only way to do this is to convert the masses (given for each option) to moles, then use coefficients see how much you will produce. note, that at STP, 1 mole of any gas is 22.4 L

OpenStudy (anonymous):

Then I believe it would be the first answer since 32g of O2 = 1 mole and for every 1 mole of O2 there are 2 moles of H20.

OpenStudy (aaronq):

that is righttt

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