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miskamm [114]
3 years ago
8

If you have 2.1 liters of hydrogen gas (at STP), what mass of hydrogen gas would you have?

Chemistry
1 answer:
GuDViN [60]3 years ago
6 0

Answer:

0.19 g

Explanation:

Step 1: Given data

Volume of hydrogen at standard temperature and pressure (STP): 2.1 L

Step 2: Calculate the moles corresponding to 2.1 L of hydrogen  at STP

At STP (273.15 K and 1 atm), 1 mole of hydrogen has a volume of 22.4 L if we treat it as an ideal gas.

2.1 L × 1 mol/22.4 L = 0.094 mol

Step 3: Calculate the mass corresponding to 0.094 moles of hydrogen

The molar mass of hydrogen is 2.02 g/mol.

0.094 mol × 2.02 g/mol = 0.19 g

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Put the steps of the carbon cycle in order using Step 1 as your starting point. Step 1: Bacteria, through nitrogen fixation and
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The answer is explained below

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The steps taking in the carbon circle using step 1 as the starting point is as follows:

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Step 2: Once nitrogen is in usable form, it is taken up by plants and assimilated into proteins.

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Step 3: An animal eats a plant and the nitrogen becomes part of the animal’s proteins.

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A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ions as
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to calculate the mole of BaSO₄

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comparing the mole ratio

1.7268 mol of BaSO₄ yields 1.7268 mol of Ba²⁺

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