Non-metals, which are organized on the right side of the periodic table, have higher electronegativity values than the metals.
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Answer:
The atom will have a negative charge.
Explanation:
Electrons are subatomic particles with a negative charge, protons are subatomic particles with a negative charge, and neutrons have no charge. When a neutral atom's balance is disrupted by an extra electron, the atom becomes negatively charged.
In a chemical reaction, 0. 3 moles of H2O result in the production of 0.2 moles of CO2. Chemical reactions are the means through which one group of chemical compounds are changed into another.
Chemical reactions are typically defined as changes that only affect the positions of electrons in the formation and breakage of chemical bonds between atoms, with no change to the nuclei (i.e., no change to the elements present). These types of changes are often included in the term chemical reactions.
Number of moles Definition We utilize this enormous quantity to measure atoms. Additionally, it equals the 6.022* 10 23 atoms that make up 12 grammes of carbon-12, or atoms.
C2H6 + 7/2O2 = 2CO2 + 3H2O,
where moles(CO2)=(2*0,3)/3=0.2 mol,
and n(CO2)=(2*0,3)/3=n(H2O);
n(CO2)=n(CO2)=n(H2O).
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Answer:
100ml of a stock 50% KNO3 solutions are needed to prepare 250ml of a 20% KNO3 solution.
Explanation:
In the given question it is mentioned that
S1=50%
V2=250ml
S2= 20%
We all know that
V1S1=V2S2
∴V1= V2×S2÷S1
∴V1= V2S2×1/S1
∴V1= 250×20÷50
∴V1= 100ml
Answer:
63.05% of MgCO3.3H2O by mass
Explanation:
<em>of MgCO3.3H2O in the mixture?</em>
The difference in masses after heating the mixture = Mass of water. With the mass of water we can find its moles and the moles and mass of MgCO3.3H2O to find the mass percent as follows:
<em>Mass water:</em>
3.883g - 2.927g = 0.956g water
<em>Moles water -18.01g/mol-</em>
0.956g water * (1mol/18.01g) = 0.05308 moles H2O.
<em>Moles MgCO3.3H2O:</em>
0.05308 moles H2O * (1mol MgCO3.3H2O / 3mol H2O) =
0.01769 moles MgCO3.3H2O
<em>Mass MgCO3.3H2O -Molar mass: 138.3597g/mol-</em>
0.01769 moles MgCO3.3H2O * (138.3597g/mol) = 2.448g MgCO3.3H2O
<em>Mass percent:</em>
2.448g MgCO3.3H2O / 3.883g Mixture * 100 =
<h3>63.05% of MgCO3.3H2O by mass</h3>
