For the following reaction, 6.79 grams of hydrogen gas are mixed with excess iodine . The reaction yields 775 grams of hydrogen iodide . hydrogen ( g ) iodine ( s ) hydrogen iodide ( g ) What is the theoretical yield of hydrogen iodide

Explanation:

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In this case, for the reaction:

As 6.79 g of hydrogen (molar mass = 2.02 g/mol) react in excess iodine, we can compute the theoretical yield of hydrogen iodide (molar mass = 127.91 g/mol)  via their 1:2 mole ratio shown on the chemical reaction:

Next, we compute the percent yield by divinding the actual yield (775 g) by the theoretical yield (860 g):

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1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.