A match can remain unlit in the middle of the flame of a bunsen burner by not having the needed substance to ignite it. The match would not have a certain amount of oxygen reaching it at the middle of the flame since almost all of the oxygen is supplied in the production of flame of the bunsen burner. Oxygen is always needed for something to burn.
2, 1, 2
Explanation:
Given equation of reaction:
Li + Br₂ → LiBr
In balancing any chemical equation, they must obey the law of conservation of matter. This law suggests that the number of moles of reactants and products must be the same in a chemical reaction.
This suggests that no amount of matter is lost during a chemical reaction.
The reaction above is a combination reaction in which two species combines to give a product.
To balance chemical reactions, we can simply inspect and assign the appropriate coefficient to the reactants and products. The coefficients should be whole numbers.
Also, the approach here would be mathematical where we would derive simple and solvable algebraic expressions to address the problem.
Assign alphabets a, b and c to the species;
aLi + bBr₂ → cLiBr
Conserving Li; a = c
Br; 2b = c
let b = 1;
c = 2
a = 2
The coefficients are 2, 1 and 2
The balanced equation is:
2Li + Br₂ → 2LiBr
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Balanced chemical equation brainly.com/question/2947744
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Dimension analysis is to be used to solve this problem. First convert 1L to milliliters. That is equivalent to 1000 ml. Then by dimension analysis, multiply the volume ( 1000ml) to the density of oil (0.92 g/ml) resulting to the answer: 920 grams.
Answer:
The molecular formula of the compound = 
The empirical formula of the compound = 
The balanced chemical equation for this reaction:
Explanation:
Compound that is 27.87% P and 72.13% S by mass and has a molar mass of 444.56 g/mol.
Molar mass of compound = 444.56 g/mol
Number of phosphorus atom = x
Number of sulfur atom = y
Atomic mass of phosphorus 31 g/mol
Atomic mass of sulfur = 32 g/mol
Percentage of element in compound :
Phosphorus :
x = 4
Sulfur :
y = 10
The molecular formula of the compound =
Empirical formula is the simplest chemical formula which depicts the whole number of atoms of each element present in the compound.
The empirical formula of the compound =
The balanced chemical equation for this reaction:
