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Igoryamba
3 years ago
8

A ______ solution contains more dissolved solute than a saturated solution at the same temperature

Chemistry
1 answer:
NeTakaya3 years ago
5 0

Answer:

i believe the answer is supersaturated  

Explanation:

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Consider the following reaction. Zn(s) 2agno3(aq) --> 2ag(s) zn(no3)2(aq)when 16. 2 g of silver was produced, _____ mole(s) o
Crazy boy [7]

The required amount of silver nitrate to produce 16.2g of silver is 25.48 grams.

<h3>What is the relation between mass & moles?</h3>

Relation between the mass and moles of any substance will be represented as:

n = W/M, where

  • W = given mass
  • M = molar mass

Moles of silver = 16.2g / 107.8g/mol = 0.15mol

From the stoichiometry of the given reaction it is clear that, same moles of silver nitrate is required to produce same moles of silver. So 0.15 moles of silver nitrate is required.

Mass of silver nitrate = (0.15mol)(169.87g/mol) = 25.48g

Hence required mass of silver nitrate is 25.48g.

To know more about mass & moles, visit the below link:

brainly.com/question/19784089

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5 0
2 years ago
I NEED HELP PLEASE!!!! CHEMISTRY QUESTION: If 38 g of Li3P and 15 grams of Al2O3 are reacted, what total mass of products will r
maksim [4K]

Answer:

21.5 g.

Explanation:

Hello!

In this case, since the reaction between the given compounds is:

2Li_3P+Al_2O_3\rightarrow 3Li_2O+2AlP

We can see that according to the law of conservation of mass, which states that matter is neither created nor destroyed during a chemical reaction, the total mass of products equals the total mass of reactants based on the stoichiometric proportions; in such a way, we first need to compute the reacted moles of Li3P as shown below:

n_{Li_3P}^{reacted}=38gLi_3P*\frac{1molLi_3P}{51.8gLi_3P}=0.73molLi_3P

Now, the moles of Li3P consumed by 15 g of Al2O3:

n_{Li_3P}^{consumed \ by \ Al_2O_3}=15gAl_2O_3*\frac{1molAl_2O_3}{101.96gAl_2O_3} *\frac{2molLi_3P}{1molAl_2O_3} =0.29molLi_3P

Thus, we infer that just 0.29 moles of 0.73 react to form products; which means that the mass of formed products is:

m_{Li_2O}=0.29molLi_3P*\frac{3molLi_2O}{2molLi_3P} *\frac{29.88gLi_2O}{1molLi_2O} =13gLi_2O\\\\m_{AlP}=0.29molLi_3P*\frac{2molAlP}{2molLi_3P} *\frac{57.95gAlP}{1molAlP} =8.5gAlP

Therefore, the total mass of products is:

m_{products}=13g+8.5g\\\\m_{products}=21.5g

Which is not the same to the reactants (53 g) because there is an excess of Li₃P.

Best Regards!

7 0
3 years ago
Jason is preparing curry from an Indian cookbook his British brother-in-law gee him for his birthday. Unfortunately, the British
Marina CMI [18]

Answer:

0.99 pounds

2,000 oz

0.423 cups

Explanation:

In order  to convert this units we need to look up their equivalences.

1 g equals 0,0022 pounds approximately

Then we need to cross-multiply:

\frac{1 g}{0.0022 pounds} = \frac{450 g}{ Xpounds} \\x = \frac{450 g x 0.0022 pounds}{1 g}

450 g equals 0.99 pounds approximately

We can do the same calculation for the other 2 ingredients

1 g equals 16 oz

Then (125 g x 16 oz) / 1 oz = 2,000 oz  (or 500 4 oz)

1 cup equals 236.59 ml

Then (100 ml x 1 cup)/ 236.59 = 0.423 cups

6 0
3 years ago
What are two methods of writing a balanced formula?
Irina-Kira [14]
Format Method - Writing the symbol of the cation and then the anion. Add whatever subscripts in order to balance the charges.

Crisscross Method - The numerical value of the charge of each ion is crossed over and becomes the subscripts for the other ion.
8 0
3 years ago
Determine the total pressure of a mixture of 0.400 mole of He and 0.600 mole of Ne in a 2.00 liter container at 25oC.
harina [27]

Answer:

Total pressure of the mixture is 12.2 atm

Explanation:

Let's apply the Ideal Gases law to solve this

Total pressure . V = Total moles . R . T

Total moles = 0.4 m of He and 0.6 mole of Ne → 1 mol

P . 2L = 1 mol . 0.082 L.atm/mol. K . 298K

P = ( 1 mol . 0.082 L.atm/mol. K . 298K) /2L

P = 12.2 atm

8 0
3 years ago
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