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Korvikt [17]
2 years ago
9

if you can’t already tell by the amount of questions i do not understand chemistry lol, giving brainliest

Chemistry
1 answer:
Vladimir [108]2 years ago
6 0

Answer:

Ok, so the process here is to convert the mass of H2 (hydrogen gas) to moles by dividing the mass by the molar mass of H2. Once you have the moles then you have to multiply by the STP (standard temperature and pressure) molar volume which should be 22.4.

Molar mass of H2 = (1.01)x2 = 2.02g/mol

19.3/2.02 = 9.55 moles

Now just multiply the moles by the molar volume

9.55 moles x 22.4 = 213.92 Litres of H2 are in 19.3g of H2

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2 years ago
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1) Write the balanced equation to state the molar ratios:

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First, convert the 250.0 L of NH3 to number of moles at STP .

Use the fact that 1 mole of gas at STP occupies 22.4 L

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Second, use the molar ratio to find the number of moles of N2 that produces 11.16 L of NH3

=> 11.16 L NH3 * [1 mol N2 / 2 mol NH3] = 5.58 mol N2

Third, convert 5.58 mol N2 into liters at STP

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What volume of hydrogen is needed to produce 2.50 mol NH3 at STP?
 

First, find the number of moles of H2 that produce 2.50 mol by using the molar ratios:

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3 years ago
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A trial of this decomposition experiment, using different quantities of reactants than those listed in the question above produc
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3 years ago
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