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3 years ago

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Chemistry

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Nataliya [291]3 years ago

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Answer:

pardon 1ve2kusura bakma

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trapecia [35]

The atoms on the products side are bonded into different molecules from the atoms on the reactants side is the chemical changes occured.

<u>Explanation:</u>

The reaction commences when the compounds on the reactant side are ready to react to give the product.
The reaction initiated by the transfer of electrons and molecules from the reactants to give the combined product of both the reactants.
It is a process on which there will be rearrangement in the structure of molecules of a substance from its physical for more chemical form.
In the above picture it shown that the red molecules combined with the white molecules additionally and changed the structure.

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3 years ago

Plsss answer my question that's on my profile pls

WINSTONCH [101]

Answer:

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3 years ago

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meriva

4. It is equal to the momentum of object 1 plus the momentum of object 2

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3 years ago

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Calculate the amount of heat required to convert 10.0 grams of ice at –20.°C to steam at 120.°C. (Sp. heat of H2O(s) = 2.09 J/g•

allsm [11]

Answer : The amount of heat required is, $3.09\times 10^4J$

Solution :

The process involved in this problem are :

$(1):H_2O(s)(-20^oC)\rightarrow H_2O(s)(0^oC)\\\\(2):H_2O(s)(0^oC)\rightarrow H_2O(l)(0^oC)\\\\(3):H_2O(l)(0^oC)\rightarrow H_2O(l)(100^oC)\\\\(4):H_2O(l)(100^oC)\rightarrow H_2O(g)(100^oC)\\\\(5):H_2O(g)(100^oC)\rightarrow H_2O(g)(120^oC)$

The expression used will be:

$\Delta H=[m\times c_{p,s}\times (T_{final}-T_{initial})]+m\times \Delta H_{fusion}+[m\times c_{p,l}\times (T_{final}-T_{initial})]+m\times \Delta H_{vap}+[m\times c_{p,g}\times (T_{final}-T_{initial})]$

where,

$\Delta H$ = heat required for the reaction

m = mass of ice = 10.0 g

$c_{p,s}$ = specific heat of solid water or ice = $2.09J/g^oC$

$c_{p,l}$ = specific heat of liquid water = $4.18J/g^oC$

$c_{p,g}$ = specific heat of gaseous water = $2.03J/g^oC$

$\Delta H_{fusion}$ = enthalpy change for fusion = $333J/g$

$\Delta H_{vap}$ = enthalpy change for vaporization = $2260J/g$

Now put all the given values in the above expression, we get:

$\Delta H=[10.0g\times 2.09J/g^oC\times (0-(-20))^oC]+10.0g\times 333J/g+[10.0g\times 4.18J/g^oC\times (100-0)^oC]+10.0g\times 2260J/g+[10.0g\times 2.03J/g^oC\times (120-100)^oC]$

$\Delta H=30934J=3.09\times 10^4J$

Therefore, the amount of heat required is, $3.09\times 10^4J$

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4 years ago

Urgent help me please answer it if you know it

Nuetrik [128]

I think it is c.

i know that plants take in co2 to then make oxygen and they need water and sunlight to grow and live.

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3 years ago

Acil lütfen. teşekkürler:)​

Acil lütfen. teşekkürler:)