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

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.