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).

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

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !