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Fiesta28 [93]
3 years ago
9

What strategies did you use when you played the balancing chemical equations game? Which atoms were the easiest to start examini

ng to try to balance the equations? And did it require trial and error?
Chemistry
2 answers:
alexandr1967 [171]3 years ago
7 0

<u>Answer:</u>

Free element is balanced at last.

We start to balance which occurs in fewer places,  first.

Balancing requires Trial and error method

<u>Balancin</u>g is making the number of atoms of each element same on both the sides  (reactant and product side).

To find the number of atoms of each element we multiply coefficient and the subscript  

For example 5 Ca_1 Cl_2 contains

5 × 1 = 5,Ca atoms and

5 × 2 = 10, Cl atoms

If there is a bracket in the chemical formula

For example 3Ca_3 (P_1 O_4 )_2 we multiply coefficient \times subscript \times number outside the bracket.......... to find the number of atoms  

(Please note: 3 is the coefficient, and if there is no number given then 1 will be the coefficient )

So

3 × 3 = 9, Ca atoms  

3 × 1 × 2 = 6, P atoms  

3 × 4 × 2 = 24, O atoms are present.

So

Let us balance the equation given

BaCl_2  + H_2 SO_4  > BaSO_4  + HCl

(Unbalanced)

Reactant side - Number of atoms of each element - Product side

1  - Ba - 1

2 - Cl - 1

2 - H - 1

1  - S - 1

4 - O - 4

So we see here H and Cl are not balanced

So by changing the coefficient of HCl as 2 we will have  

BaCl_2+ H_2 SO_4  > BaSO_4+2HCl

(Balanced)  

Reactant side - Number of atoms of each element - Product side

1  - Ba - 1

2 - Cl - 2

2 - H - 2

1  - S - 1

4 - O - 4

So we see the number of atoms of each element is same on both the sides.

Hence the equation is balanced !!!!!!!!!!

Yakvenalex [24]3 years ago
3 0

<u>Answer:</u>

<em>Latest take an example to understand how </em><em>balancing of chemical reaction</em><em> is done that is assuming the reaction between iron as well as </em><em>oxygen which reacts to form rust.</em>

<u>Explanation:</u>

For this we would simply right the reactant and product that is expected. Then we would see the number of molecules of each element present on either side.

If in the reaction the element’s molecules are the same on both sides then the reaction would be correct and if not then we have to apply trial and error method to balance the equation such that the number of molecules of each element is equal on both sides of the reaction.

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<h3>What is Density ?</h3>

Density is defined as mass per unit volume. S.I unit if density is kg/m³.

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Density = \frac{\text{Mass}}{\text{Volume}}  or d = \frac{m}{V}

<h3>What is Intensive Property ? </h3>

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Disclaimer: The given question is incomplete on the portal. Here is the complete question.

Question: The density (d) of a substance is an intensive property that is defined as the ratio of its mass (m) to its volume (v)

density = \frac{\text{Mass}}{\text{Volume}}  or d = \frac{m}{V}

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How many grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C?
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Answer:

22.656 grams of oxygen gas are there in a 2.3L tank at 7.5 atm and 24° C

Explanation:

An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law:

P * V = n * R * T

where R is the molar constant of the gases and n the number of moles.

In this case you know:

  • P= 7.5 atm
  • V= 2.3 L
  • n= ?
  • R= 0.082 \frac{atm*L}{mol*K}
  • T= 24 °C= 297 °K (being 0°C=273°K)

Replacing:

7.5 atm* 2.3 L=n*0.082 \frac{atm*L}{mol*K} *297K

Solving:

n=\frac{7.5 atm* 2.3 L}{0.082 \frac{atm*L}{mol*K} *297K}

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Knowing that oxygen gas is a diatomic gas of molecular form O₂ and its mass is 32 g / mole, you can apply the following rule of three: if 1 mole contains 32 grams, 0.708 moles, how much mass will it have?

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