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Andrew [12]
3 years ago
8

Balance the following reaction. A coefficient of "1" is understood. Choose option "blank" for the correct answer if the coeffici

ent is "1". KNO3 → KNO2 + O2
Chemistry
2 answers:
Roman55 [17]3 years ago
5 0
2KNO3 -> 2KNO2 + O2. Hope this helps!
zalisa [80]3 years ago
5 0

Answer: 2KNO_3\rightarrow 2KNO_2+O_2

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

The balanced equation will be:

2KNO_3\rightarrow 2KNO_2+O_2

The atoms on reactant and product side must be same.

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How to find change in enthalpy
arlik [135]
∆H = m x s x ∆T, where m is the mass of the reactants, s is the specific heat of the product, and ∆T is the change in temperature from the reaction.
5 0
2 years ago
"calculate the ratio of the velocity of hydrogen molecules to the velocity of carbon dioxide molecules at the same temperature"
Ne4ueva [31]

Answer: 1:4.69

Explanation:

The ratio can be expressed as:

Ua/Ub= √(Mb/Ma)

Where Ua/Ub is the ratio of velocity of hydrogen to carbon dioxide and Ma is the molecular mass of hydrogen gas= 2

Mb is the molecular mass of CO2 = 44

Therefore

Ua/Ub= √(44/2)

Ua/Ub = 4.69

Therefore the ratio of velocity of hydrogen gas to carbon dioxide = 1:4.69

which implies hydogen is about 4.69 times faster than carbon dioxide.

8 0
3 years ago
Can a nonpolar molecule contain polar covalent bonds?
Serggg [28]
Yes they can have a trace of polar in them
3 0
3 years ago
A chemical reaction can theoretically produce 137.5 grams of product, but in actuality 112.9 grams are
Butoxors [25]
<h3>Answer:</h3>

82.11%

<h3>Explanation:</h3>

We are given;

  • Theoretical mass of the product is 137.5 g
  • Actual mass of the product is 112.9 g

We are supposed to calculate the percentage yield

  • We need to know how percentage yield is calculated;
  • To calculate the percentage yield we get the ratio of the actual mass to theoretical mass and express it as a percentage.

Thus;

% yield = (Actual mass ÷ Experimental mass) × 100%

            = (112.9 g ÷ 137.5 g) × 100%

            = 82.11%

Therefore, the percentage yield of the product is 82.11 %

7 0
3 years ago
I'd: 9872093250, password: qqqqq, join the meeting​
Sonja [21]
You keep on saying join fast wdym?!
4 0
2 years ago
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