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kotegsom [21]
3 years ago
15

Why do we put these three words together in the 'fire triangle'?

Chemistry
1 answer:
bazaltina [42]3 years ago
7 0
The three word of this is to represent what it takes to create and maintain a fire
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Explanation:

The paper clip allows elictricity to pass, unlike the eraser or paper

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Help me with this attachment please​
Anna007 [38]

Answer:

See explanation

Explanation:

Let us recall that the basic rule in writing balanced chemical reaction equations is that the number of atoms of each element on the right hand side of the reaction equation is the same of the number of atoms of the same element on the left hand side of the reaction equation.

The reaction of red hot iron and steam is written as follows;

3Fe + 4H2O → Fe3O4 + 4H2.

The decomposition reaction of ammonium dichromate is written as;

(NH4)2Cr2O7 → N2 + Cr2O3 + 4H2O

Reaction of aluminium, sodium hydroxide and water is as follows,

2Al + 2NaOH + 2H2O ----> 2NaAlO2 + 3H2

Reaction of potassium bicarbonate with sulphuric acid;

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Reaction of zinc and sodium hydroxide is as follows;

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5 0
3 years ago
Which kind of material would best accomplish this task ?
timofeeve [1]
What's the question ?
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3 years ago
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What is the half-life of a first-order reaction if it takes 4.4 x 102 seconds for the concentration to decrease from 0.50 M to 0
elena55 [62]

Answer: The half-life of a first-order reaction is, 3.3\times 10^2s

Explanation:

All the radioactive reactions follows first order kinetics.

Rate law expression for first order kinetics is given by the equation:

k=\frac{2.303}{t}\log\frac{[A_o]}{[A]}

where,  

k = rate constant = ?

t = time taken = 440 s

[A_o] = initial amount of the reactant = 0.50 M

[A] = left amount =  0.20 M

Putting values in above equation, we get:

k=\frac{2.303}{440s}\log\frac{0.50}{0.20}

k=2.083\times 10^{-3}s^{-1}

The equation used to calculate half life for first order kinetics:

t_{1/2}=\frac{0.693}{k}

Putting values in this equation, we get:

t_{1/2}=\frac{0.693}{2.083\times 10^{-3}s^{-1}}=332.69s=3.3\times 10^2s

Therefore, the half-life of a first-order reaction is, 3.3\times 10^2s

4 0
3 years ago
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