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3 years ago

Why is carbon dioxide used in fire extinguisher?

2 answers:

3 0

As Fire needs oxygen to burn, Carbon Dioxide Covers the fire like an blanket and cuts the contact of fire to the oxygen present in the air, So Fire stops burning.That is why Carbon Dioxide is Considere as the best Fire Extinguisher.

Zinaida [17]3 years ago

3 0

Answer:Carbon dioxide extinguishes work by displacing oxygen, or taking away the oxygen element of the fire triangle. The carbon dioxide is also very cold as it comes out of the extinguisher, so it cools the fuel as well

Explanation:

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What's the force between two moving objects that are touching called

m_a_m_a [10]

I think it is friction.

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4 years ago

Consider the decomposition of hydrogen peroxide reaction. If the rate of decomposition of hydrogen peroxide at a particular temp

Natasha2012 [34]

Answer:

0.049 mol/L.s

Explanation:

The decomposition of hydrogen peroxide is:

$H_2O_2 \to H_2O + \dfrac{1}{2}O_2$

$Rate = -\dfrac{\Delta [H_2O_2]}{\Delta t}= \dfrac{\Delta [H_2O_2]}{\Delta t}= \dfrac{ 2 \Delta [H_2O_2]}{\Delta t}$

The rate of decomposition reaction = the rate of formation of $H_2O$ = 0.098 mol/L.s

∴

Rate of formation of $O_2$ $= \dfrac{ rate \ of \ reaction }{2}$

$= \dfrac{ 0.098 }{2}$

= 0.049 mol/L.s

8 0

3 years ago

For a concentration technique, Stotal is given as 19.31 ± 0.035, Smb is 0.22 ± 0.008, and kA is 0.154 ± 0.007 ppm–1, where Stota

professor190 [17]

Answer:

Explanation:

8 0

3 years ago

Determine the molar mass of CuSO4 (the solute) in a 1.0M aqueous solution of CuSO4

inna [77]

Answer:

See explanation.

Explanation:

Hello,

In this case, we could have two possible solutions:

A) If you are asking for the molar mass, you should use the atomic mass of each element forming the compound, that is copper, sulfur and four times oxygen, so you can compute it as shown below:

$M_{CuSO_4}=m_{Cu}+m_{S}+4*m_{O}=63.546 g/mol+32.00g/mol+4*16.00g/mol\\\\M_{CuSO_4}=159.546g/mol$

That is the mass of copper (II) sulfate contained in 1 mol of substance.

B) On the other hand, if you need to compute the moles, forming a 1.0-M solution of copper (II) sulfate, you need the volume of the solution in litres as an additional data considering the formula of molarity:

$M=\frac{n_{solute}}{V_{solution}}$

So you can solve for the moles of the solute:

$n_{solute}=M*V_{solution}$

Nonetheless, we do not know the volume of the solution, so the moles of copper (II) sulfate could not be determined. Anyway, for an assumed volume of 1.5 L of solution, we could obtain:

$n_{solute}=1mol/L*1.5L=1.5mol$

But this is just a supposition.

Regards.

4 0

3 years ago

Calculate the percentage by mass of nitrogen in ptcl2(nh3)2.

Sav [38]

Molar Mass: 300.0510 g/mol

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3 years ago