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Sodium amide, known commercially as sodamide, is used in preparing indigo, the dye used to color blue jeans. It is an ionic compound with the formula $mathrm{NaNH}_...

Question

Sodium amide, known commercially as sodamide, is used in preparing indigo, the dye used to color blue jeans. It is an ionic compound with the formula $mathrm{NaNH}_{2}$. What is the electrondot formula of the amide anion, $mathrm{NH}_{2}^{-}$ ?

Sodium amide, known commercially as sodamide, is used in preparing indigo, the dye used to color blue jeans. It is an ionic compound with the formula $mathrm{NaNH}_{2}$. What is the electrondot formula of the amide anion, $mathrm{NH}_{2}^{-}$ ?



Answers

Sodium amide, known commercially as sodamide, is used in preparing indigo, the dye used to color blue jeans. It is an ionic compound with the formula $\mathrm{NaNH}_{2}$. What is the electrondot formula of the amide anion, $\mathrm{NH}_{2}^{-}$ ?

The common name for NH three is ammonia. Do that? This is a common name. What would it systematic name be? It's systematic name. It's named after the elements present. It's nitrogen. Try hydride. This would be the systematic name for NH three. There's one nitrogen. We don't read the prefix mono in front, so it's not mono nitrogen. Just nitrogen for a single atom. Listed first, there's three hydrogen atoms tries the prefix for three tri hydrate. So the systematic name for NH three is nitrogen tri hydride, right?

In this question were given to compounds that have both sold even nitrogen but that are differing by their percent masses of each elements and were asked to find the empirical formula of each compound. So first, we're gonna assume that we have 100 grams of this compound so we can convert these percentages and to the masses. Next, we want to convert these into moles. So we know that sodium has a molar mass of 22.99 grams from all. And so 83.12 grams of this would be 3.63 moles of sodium. Similarly nitrogen with the molar mass of 14.0 grams from all has 1.21 moles in this compound. Now, to get whole numbers, we're gonna want to divide by the lowest number, which in this case is 1.21 And by doing this, we find that we have three moles of sodium for every one mole of 19 in compound one. So Compound one has an empirical formula of n a three end. Now we're going to go ahead and do this for compound to again. We're assuming that we have 100 grams ever gonna convert these two moles and we're gonna divide by the lowest number. And we find that for every mole of sodium, there are three moles of nitrogen which makes our empirical formula for compound to and a n three.

The cobalt that is violet that is found in a compound that has a cobalt with a two plus charge combined with the an ion phosphate, which we know has a three minus charge is going to require in order to have a neutral Ionic compound. Three Cobalts for every two faucets or C 03 p 04 peel foreign brackets, two of them.

This question is a combination of using the ideal gas law and determining the empirical formula through mass percent. So let's start with determining the empirical formula through mass percent. If it's 11.79% carbon, then if we have 100 g of the material, we would have 11.79 g of carbon, which we can convert into moles of carbon by dividing by its smaller mass. If it's 69.57% chlorine than 100 g of the compound would contain 69.57 g chlorine, which we can convert two moles by divided by chlorine. Smaller mass. Then, if we sum up the two percentages that were given to us and subtract them from 100 what will be left over will be the percent that is Floren, which ends up being 18.64 We divide those grams by the molar mass of floor een in order to get the moles floor een. These then become the moles that air present in 100 g of the sample. If we divide by the smallest, we can then convert them toe whole numbers and we'll get one more grant are one mole carbon, two moles, chlorine and one mole florin. So the empirical formula is CCL two af Now we can use the ideal gas law in order to determine the moles. We'll take the pressure given to us in millimeters of mercury converted into atmospheres. This is our pressure value will multiply it by the leaders and then divide by rt. The universal gas constant and the temperature in kelvin temperature was given to us in Celsius. We just converted it to to 98.15 Calvin and we get 5.24 times 10 to the negative four moles of the compound. If we have that many moles in 0.107 g of the compound, we can calculate the molar mass or the Yeah, the molar mass of the compound by taking the mass that corresponds to the moles that we determined from our ideal gas law that gives us a Moeller mass of 204.5 g per mole. The molar mass of the empirical formula was one on one point 01 g. So it appears that the, uh, molecular formula is going to be twice the empirical formula so we can get the actual Mueller Mass of the compound or C two c l four f two.


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