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3 years ago

Which element is used to reduce metal oxides and make pure metals?

Chemistry

1 answer:

Setler [38]3 years ago

5 0

Can vary. Carbon is used quite commonly, and extracts metal oxides, works with zinc, iron, tin, lead and copper.

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How did rutherford's experimental evidence lead to the development of a new atomic number

borishaifa [10]

Rutherford's experiment was the gold foil experiment.

The gold foil experiment was him shooting alpha particles (you could think of this as a Helium atom without its electrons) into a gold foil. The whole experiment was surrounded with something called Zinc Sulfide which sparked when the alpha particles hit it.

Most of the alpha particles went through, approximately 1 in 8000 alpha particles deflected at a large angle (almost right back to where it was shot).

This constant ratio caused him to conclude that:-the atom was mostly empty space (since most alpha particles went through)-there was something very positive in the atom (the proton)-the proton was very dense (since it made something going light speed deflect back at a large angle)-The proton was also very small (since only 1 in 8000 hit it)

Prior to the discovery of the proton, John Dalton's periodic table was used. Having "elements" such as soda and potash. Now that we have discovered the proton and found out that each atom's number of protons is unique, we used that to classify each element's identity.

8 0

4 years ago

How many protons, electrons, and neutrons does a magnesium-25 atom have if it has a sharge=2?

Sveta_85 [38]

Answer:

There are 12 protons, and 10 electrons in an Mg2+ ion, the normal amount of neutrons is 12.

Explanation:

3 0

3 years ago

A hydrated sample weighing 20.0 g is heated in a crucible at 250°C. After cooling the sample now has a weight of 16.5 g.

anzhelika [568]

Given parameters:

Weight of hydrated sample = 20g

Temperature = 250°C

Weight after cooling = 16.5g

Unknown:

Weight of water lost from the sample = ?

Solution:

The weight of water lost from the sample;

Weight of water lost = Weight of hydrated sample - Weight of dry sample

Weight of water lost = 20g - 16.5g = 3.5g

% of water in the sample = $\frac{mass of water}{mass of original sample} x 100$

Input parameters solve;

= $\frac{3.5}{20} x 100$

=17.5%

8 0

3 years ago

How has everyone been and nice to meet whoever else get's on here.

jeka57 [31]

Answer:

Hello everyone and thnx for points

Explanation:

6 0

3 years ago

A 2.950Ã—10âˆ’2 M solution of glycerol (C3H8O3) in water is at 20.0âˆ˜C. The sample was created by dissolving a sample of C3H8O3

lina2011 [118]

Answer:

a. 2.959x10⁻²m

b. 5.327x10⁻⁴

c. 0.272%

d. 2718 PPM

Explanation:

A solution of 2.950x10⁻²M contains 2.950x10⁻² moles of Glycerol per Liter of solution. As the volume of the solution made was 1.000L, moles of glycerol are 2.950x10⁻².

a. molality: Molality is defined as the ratio between moles of solute (2.950x10⁻²) in kg of solvent. As there are 998.7mL of solvent and density is 0.9982g/mL, kg are:

998.7mL ₓ (0.9982g/mL) ₓ (1kg / 1000g) = 0.9969kg of solvent.

Molality: 2.950x10⁻² moles / 0.9969kg of solvent = 2.959x10⁻²m

b. Mole fraction is the ratio between moles of solute and total moles. Moles of water are:

998.7mL ₓ (0.9982g/mL) ₓ (1mol / 18.01g) = 55.35 moles of water.

Mole fraction glycerol:

2.950x10⁻² moles / (2.950x10⁻²moles + 55.35) = 5.327x10⁻⁴

c. Percent by mass Is the ratio by mass of solute and solution multiplied 100 times.

Mass of glycerol (Molar mass: 92.09g/mol):

2.950x10⁻² moles × (92.09g / mol) = 2.717g of glycerol

Mass of water:

998.7mL ₓ (0.9982g/mL) = 996.9g of water.

Percent by mass:

2.717g of glycerol / (996.9g of water + 2.717g) × 100 = 0.272%

d. Parts per million are defined as the ratio between mg of solute and kg of solution.

mg of 2.717g of glycerol are 2717mg

kg of solution are (996.9g + 2.717g) / 1000 = 0.9996kg

Parts per million:

2717mg / 0.9996kg = 2718 PPM

4 0

3 years ago