How many grams of CsXeF7 can be produced from the reaction of 15.2 grams of CsF and 260 grams of XeF6?

39.72 g

Explanation:

Given data:

Mass of CsF = 15.2 g

Mass of XeF₆ = 260 g

Mass of Cs[XeF₇] = ?

Solution:

Chemical reaction:

CsF + XeF₆   →  Cs[XeF₇]

Number of moles of CsF:

Number of moles = mass/ molar mass

Number of moles = 15.2 g/151.9 g/mol

Number of moles = 0.1 mol

Number of moles of XeF₆ :

Number of moles = mass/ molar mass

Number of moles = 260 g/245.28 g/mol

Number of moles = 1.06 mol

Now we will compare the moles of Cs[XeF₇] with both reactants.

                            CsF               :            Cs[XeF₇]

                               1                 :                 1

                             0.1                :              0.1

                             XeF₆            :           Cs[XeF₇]

                                 1               :               1

                                1.06           ;              1.06

Number of moles of Cs[XeF₇] produce by  CsF are less so it will limiting reactant and limit the yield of Cs[XeF₇].

Mass of Cs[XeF₇]:

Mass = number of moles × molar mass

Mass = 0.1 mol × 397.2 g/mol

Mass = 39.72 g

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.