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maksim [4K]
2 years ago
13

What is the volume occupied by 3.00 mol of hydrogen gas at STP? *

Chemistry
1 answer:
xxTIMURxx [149]2 years ago
6 0

Answer: V=67.2 L

Explanation:

For this problem we will need to use the Ideal Gas Law.

Ideal Gas Law: PV=nRT

P=1.00 atm (STP)

V=?

n=3.00 mol

R=0.08206Latm/Kmol

T=273.15 K (STP)

To find V, we would manipulate the equation to V=nRT/P

V=\frac{(3.00 mol)(0.08206Latm/Kmol)(273.15K)}{1.00 atm}

V=67.244 L

With significan figures, our answer is V=67.2 L.

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The answer is a change in internal energy causes work to be done and heat to flow into the system.  

<u>Explanation:</u>

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This problem is providing the chemical reaction whereby barium nitride reacts with water to produce barium hydroxide and ammonia, so the number of moles of barium nitride are required in order to produce 8.3 moles of ammonia. It asks for us to evaluate the student's setup, so we conclude the answer is C. "1 mol of NH3 should be replaced with 2 mol of NH3", according to:

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In chemistry, stoichiometric calculations are used to figure out the moles or mass of a substance, given information about another one in the reaction. In this case, for the given chemical equation:

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