Xenon hexafluoride (XeF6) reacts with hydrogen gas (H2) to produce xenon gas and hydrogen fluoride gas (HF) according to the following chemical equation. XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g) If 1.74 moles of H2 is consumed in the chemical reaction above, how many grams of H2 are consumed? For your answer, only type in the numerical value with three significant figures. Do NOT include the unit or the chemical (numbers only).

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jufsanabriasa jufsanabriasa · Answer 1 · 2020-09-10T02:29:00+02:00

Answer:

3.52g

Explanation:

As you know from the question, 1.74 moles of hydrogen, H₂, are reacting (Moles consumed). The question is about the grams that are consumed.

To convert moles to grams of substance, you must use molar mass:

Molar mass of H₂ is twice atomic mass of hydrogen (H = 1.008g/mol; H₂ = 2.016g/mol).

1.74 moles of H₂ are:

1.745 moles * (2.016g / mol) =

3.52g

Answer without unit: 3.52

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lhmarianaramalho lhmarianaramalho · Answer 2 · 2022-01-28T11:19:06+01:00

3.50 grams of H2 are consumed in the reaction.

To calculate the amount of grams present in a given amount of mole of an element, it is necessary to use the molar mass.

In this case the molar mass of hydrogen corresponds to:

[tex]MM_{H} = 1.008 g/mol[/tex]

Thus, the molar mass of [tex]H_{2}[/tex] is equal to:

[tex]MM_{H}_{2} = 2.016 g/mol[/tex]

Finally, the amount of mass for one mole must be related to the number of moles given, so that:

[tex]\frac{1mole}{1.74moles} =\frac{2.016grams}{xgrams}[/tex]

[tex]x = 3,50[/tex]

So, 3.50 grams of H2 are consumed in the reaction.

Learn more about mole calculation in: brainly.com/question/15209553