Mass of Magnesium bromide : 5.76 g
<h3>Further explanation</h3>
Complete question
<em>What mass of Magnesium bromide is formed when 1.00 g of magnesium reacts with 5.00 g of bromine?</em>
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Reaction
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mol Mg
![\tt \dfrac{1}{24}=0.042](https://tex.z-dn.net/?f=%5Ctt%20%5Cdfrac%7B1%7D%7B24%7D%3D0.042)
mol Br₂
![\tt \dfrac{5}{160}=0.0313](https://tex.z-dn.net/?f=%5Ctt%20%5Cdfrac%7B5%7D%7B160%7D%3D0.0313)
Limiting reactants : Br₂(smaller)
mol MgBr₂ = mol Br₂=0.0313
mass MgBr₂ :
![\tt 0.0313\times 184,113 =5.76~g](https://tex.z-dn.net/?f=%5Ctt%200.0313%5Ctimes%20184%2C113%20%3D5.76~g)
Answer:
its d, the explanation for this is because I need some more points so ima go ahead and just spam random questions
Answer:To calculate the Molarity of a 70 wt. % Nitric Acid the number of moles of HNO 3 present in 1 liter of acid needs to be calculated. Knowing the density of the acid to be 1.413 g/mL, we can calculate the weight of 1 L of 70% HNO 3 to be 1413
Explanation:
If my memory serves me well, each period in the periodic table corresponds to a principal energy level. I think it's correct because periods are the horizontal rows and when you go down you always add <span> one to the principal energy level. Hope it is clear. Good luck!</span>
It's the second one. cause u have to add