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3 years ago

Alchemist made which of the following contributions to the development of chemistry?

1 answer:

6 0

Alchemists advanced the tools and procedures for working with chemicals. Alchemists also developed methods for sorting out mixtures and cleansing chemicals. They designed equipment that is still in use today including beakers, flasks, tongs, funnels, and the mortar and pestle. Also, Alchemists backed to an unbelievable variety of what would later be acquainted as chemical industries: basic metallurgy, metalworking, the invention of inks, dyes, paints, and cosmetics, leather-tanning, and the preparation of extracts and liquors.

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using the equation 2h2+o2-->2h2o if 192g of oxygen are produced how many grmas of hydrogen must react with it

Brilliant_brown [7]

Equation: 2H₂ + O₂ → 2H₂O

Now, Given mass of Oxygen = 192 g
Molar mass of Oxygen = 16 g/mol

No. of moles in Oxygen = 16/192 = 0.0833

Now, for every mole of Oxygen, 2 mole of Hydrogen will form,
so, Number of moles of Hydrogen = 0.0833 * 2 = 0.167

Given mass = Number of Moles * Molar mass
Given mass = 0.167 * 2
m = 0.33 g

In short, Your Answer would be: 0.33 g

Hope this helps!

7 0

3 years ago

Read 2 more answers

Compared to a solution with a ph of 6, the hydronium ion concentration of a solution with a Ph of 4 has how many more times the

Alexxx [7]

Answer: The hydronium ion concentration of a solution with a pH of 4 is 100 times more than the the hydronium ion concentration of a solution with a pH of 6

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

$pH=-\log [H^+]$

1. Solution with pH of 6

$6=-\log [H^+]$

$[H^+]=10^{-6}$

2. Solution with pH of 4

$4=-\log [H^+]$

$[H^+]=10^{-4}$

$\frac{H^+_4}{H^+_6}=\frac{10^{-4}}{10^{-6}}=10^{2}={100}$

${H^+_4}=100\times {H^+_6}$

Thus the hydronium ion concentration of a solution with a pH of 4 is 100 times more than the the hydronium ion concentration of a solution with a pH of 6

5 0

3 years ago

Calculate the number of atoms of each 4(NH4)2S

vaieri [72.5K]

4- N
8- H
2-S
Or in 4 nitrogens, 8 hydrogens, and 2 silicons

3 0

3 years ago

Calculate the Experimental Molar Volume in L/mol of the Hydrogen gas, H2, if the volume of H2 at STP is 52.8 mL and the mass of

lana66690 [7]

Answer:

The Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol

Explanation:

We are given that

Volume of H2 at STP=52.8mL

Mass of magnesium metal ,M(Mg)=0.055g

We have to find the Experimental Molar Volume in L/mol of the Hydrogen gas.

Molar mass of Mg=24.305 g/mol

Number of moles= $\frac{given\;mass}{molar\;mass}$

Using the formula

Number of moles of Mg= $\frac{0.055}{24.305}$ moles

Number of moles of Mg=0.00226moles

Number of moles of Mg=Number of moles of H2

Number of moles of H2=0.00226moles

Molar volume of Hydrogen gas (H2)= $\frac{volume\;at\;STP}{No\;of\;moles\;H_2}$

Molar volume of Hydrogen gas (H2)= $\frac{52.8}{0.00226}mL/mol$

Molar volume of Hydrogen gas (H2)= $\frac{52.8}{0.00226}\times 10^{-3}L/mol$

$1L=1000mL$

Molar volume of Hydrogen gas (H2)=23.36L/mol

Hence, the Experimental Molar Volume in L/mol of the Hydrogen gas=23.36L/mol

6 0

3 years ago

An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has

hichkok12 [17]

The answer is (4) a total of eight valence electrons. The valence electrons are defined as electrons that are mostly like to be involved in a chemical reaction. So the Argon is stable because the 8 valence electrons is already a stable state.

3 0

4 years ago