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3 years ago

How can balancing equations support the law of conservation

Chemistry

1 answer:

amm18123 years ago

4 0

Answer:

detail is given below.

Explanation:

This law was given by French chemist Antoine Lavoisier in 1789. According to this law mass of reactant and mass of product must be equal, because masses are not created or destroyed in a chemical reaction.

Law of conservation of mass:

According to the law of conservation mass, mass can neither be created nor destroyed in a chemical equation.

For example:

In given photosynthesis reaction:

6CO₂ + 6H₂O → C₆H₁₂O₆ + 6O₂

The given equation is balanced chemical equation of photosynthesis. There are six carbon atoms, eighteen oxygen atoms and twelve hydrogen atoms on the both side of equation so this reaction followed the law of conservation of mass.

If equation is not balanced,

CO₂ + H₂O → C₆H₁₂O₆ + O₂

It can not follow the law of conservation of mass because mass is not equal on both side of equation.

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Which answer correctly ranks the atoms in terms of decreasing electronegativity (the highest electronegativity first)? which ans

Degger [83]

Answer:

O, N, C, H

Explanation:

Electronegativity of an element is the property that combines the ability of its atom to lose or gain electrons. It measures the relative tendency with which the atoms of the element attracts valence electrons in a chemical bond.

On the periodic table, Electronegativity increases across the period but decreases down a group.

To solve the given problem, let us use thE Pauling's table of electronegativities to compare the electronegativities of the elements.

On the table:

C = 2.5

H = 2.1

O = 3.5

N = 3.0

In terms of decreasing electronegativities, the atoms are arranged as:

O N C H

4 0

3 years ago

Rank and explain how the freezing point of 0.100 m solutions of the following ionic electrolytes compare. List from lowest freez

Elden [556K]

Answer:

The solutions are listed from the lowest freezing point to highest freezing point.

Mg₃(PO₄)₂ - AlBr₃ - BeBr₂ - KBr

Explanation:

Colligative property of freezing point, is the freezing point depression.

Formula is:

ΔT = Kf . m . i

Where ΔT = T° freezing pure solvent - T° freezing solution

Kf is the cryoscopic constant

m is molality and i is the Van't Hoff factor (number of ions, dissolved in solution)

In this case, T° freezing pure solvent is 0° because it's water, so the Kf is 1.86 °C/m, and m is 0.1 molal.

The i modifies the T° freezing solution. The four salts, are ionic compounds, so for each case:

BeBr₂ → Be²⁺ + 2Br⁻ i = 3

AlBr₃ → Al³⁺ + 3Br⁻ i = 4

Mg₃(PO₄)₂ → 3Mg²⁺ + 2PO₄⁻³ i = 5

KBr → K⁺ + Br⁻ i = 2

Solution of Mg₃(PO₄)₂ will have the lowest temperature of freezing and the solution of KBr, the highest (always lower, than 0°).

8 0

3 years ago

1. How many molecules are equal to 1x10(-5) moles?

tangare [24]

Answer:

10×(-5)=-50 which means their are -50 moles

4 0

2 years ago

PH CHEM, PLEASE HELP QUICK! NO LINKS/VIRUSES PLEASE!

Contact [7]

Answer:

The pH of the solution is 11.48.

Explanation:

The reaction between NaOH and HCl is:

NaOH + HCl → H₂O + NaCl

From the reaction of 3.60x10⁻³ moles of NaOH and 5.95x10⁻⁴ moles of HCl we have that all the HCl will react and some of NaOH will be leftover:

$n_{NaOH}} = n_{i_{NaOH}} - n_{HCl} = 3.60 \cdot 10^{-3} moles - 5.95 \cdot 10^{-4} moles = 3.01 \cdot 10^{-3} moles$

Now, we need to find the concentration of the OH⁻ ions.

$[OH^{-}] = \frac{n_{NaOH}}{V}$

Where V is the volume of the solution = 1.00 L

$[OH^{-}] = \frac{n_{NaOH}}{V} = \frac{3.01 \cdot 10^{-3} moles}{1.00 L} = 3.01 \cdot 10^{-3} mol/L$

Finally, we can calculate the pH of the solution as follows:

$pOH = -log([OH^{-}]) = -log(3.01 \cdot 10^{-3}) = 2.52$

$pH + pOH = 14$

$pH = 14 - pOH = 14 - 2.52 = 11.48$

Therefore, the pH of the solution is 11.48.

I hope it helps you!

3 0

3 years ago

Help ASAP please someone

AfilCa [17]

Can u plz give more information

7 0

3 years ago