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olga55 [171]
2 years ago
14

How many moles of NaOH are required to prepare 2.90 L of 1.8 M NaOH?

Chemistry
2 answers:
vfiekz [6]2 years ago
5 0
Here is a couple of useful formula to use when you get problems like this.

Molarity= \frac{moles}{Liters}        ----->      moles=  (Molarity) x (Liters)

since they are asking for moles, we are using the one on the right. 

Molarity= 1.8 M
Liters= 2.90 L

moles= (1.8 M) x (2.90 L)= 5.2 moles of NaOH


marusya05 [52]2 years ago
3 0
V=2.90 L
c=1.8 mol/L

n(NaOH)=vc

n(NaOH)=2.90L*1.8mol/L=5.22 mol
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The empirical formula of the following compounds 0.903 g of phosphorus combined with 6.99 g of bromine.

<h3>What is empirical formula?</h3>

The simplest whole number ratio of atoms in a compound is the empirical formula of a chemical compound in chemistry. Sulfur monoxide's empirical formula, SO, and disulfur dioxide's empirical formula, S2O2, are two straightforward examples of this idea. As a result, both the sulfur and oxygen compounds sulfur monoxide and disulfur dioxide have the same empirical formula.

<h3>How to find the empirical formula?</h3>

Convert the given masses of phosphorus and bromine into moles by multiplying the reciprocal of their molar masses. The molar masses of phosphorus and bromine are 30.97 and 79.90 g/mol, respectively.

Moles phosphorus = 0.903 g phosphorus \frac{mol phosphorus}{ 30.97 g phosphorus}= 0.0293 mol

Moles bromine 6.99 g bromine\frac{mol bromine}{79.90 g bromine}=0.0875 mol

The preliminary formula for compound is P0.0293Bro.0875. Divide all the subscripts by the subscript with the smallest value which is 0.0293. The empirical formula is P1.00Br2.99 ≈ P₁Br3 or PBr3

To learn more about empirical formula visit:

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#SPJ4

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