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Semmy [17]
3 years ago
11

A student used 10 mL water instead of 30mL for the extraction of the NaCl from the mixture. How would this affect the calculated

percentage of NaCl in the sample?
Chemistry
1 answer:
leonid [27]3 years ago
5 0
In this problem, the solute is sodium chloride, the salt while the solvent which comprise of a larger mass in the solution is water. When the solvent volume is decreased which is related to its mass, with the solute mass being held constant, then the concentration of salt increases. This is called concentration method. 
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nadya68 [22]

Answer: Glucose is a simple sugar with six carbon atoms and one aldehyde group.

Explanation: hope this helps you

4 0
3 years ago
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Write the formula for each compound
nalin [4]

Answer:

Chromium(III) Sulfite Cr2(SO3)3 Molecular Weight

Mg(ClO)2 - PubChem

Ni(NO3)2

5 0
3 years ago
Solid iron(III) hydroxide decomposes to produce iron(III) oxide and water vapor. If 0.75 L of water vapor is produced at STP, ho
MaRussiya [10]
The reaction is 2Fe(OH)3 --> Fe2O3 + 3H2O, so the mole ratio of iron (III) hydroxide to water is 2 to 3, or 0.667. That means you need 0.667 moles of iron(III) hydroxide for every mole of water that forms. 

<span>You are missing some info. You need the volume of the water vapor. At STP, 1 Liter of gas contains 22.4 moles, so you can find the moles of water vapor once you know the volume of the water vapor in Liters. </span>

<span>Then, mulitply moles of water by 0.667 to find moles of iron (III) hydroxide used. Finally, multiply by the molar mass of iron (III) hydroxide to find the mass in grams.</span>
8 0
4 years ago
How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a
ira [324]

Answer:

38 L

Explanation:

There is some info missing. I think this is the original question.

<em>Consider the chemical reaction: C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g). How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K.</em>

<em />

Step 1: Write the balanced equation

C(s) + H₂ O(g) ⟶ CO(g) + H₂ (g)

Step 2: Calculate the moles corresponding to 15.2 g of C

The molar mass of C is 12.01 g/mol.

15.2g \times \frac{1mol}{12.01g} = 1.27 mol

Step 3: Calculate the moles of H₂ produced from 1.27 moles of C

The molar ratio of H₂ to C is 1:1. The moles of H₂ produced are 1/1 × 1.27 mol = 1.27 mol.

Step 4: Calculate the volume of H₂

We will use the ideal gas equation.

P \times V = n \times R \times T\\V = \frac{n \times R \times T}{P} = \frac{1.27mol \times \frac{0.0821atm.L}{mol.K}  \times 360K}{1.0atm}= 38 L

3 0
4 years ago
What is the atomic mass of an element is equal to?
Tatiana [17]
Protons and Neutrons is what determines the atomic mass. I cannot further explain this answer, however, I hope I helped!
6 0
3 years ago
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