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solmaris [256]
2 years ago
8

Consider the chemical equations shown here.

Chemistry
1 answer:
vichka [17]2 years ago
5 0

P₄0₆_{s} + 20₂_{g}   ⇒    P₄0₁₀_{s}

Explanation:

The overall equation for the reaction that produces  P₄0₁₀ is :

P₄0₆_{s} + 20₂_{g}   ⇒    P₄0₁₀_{s}

Now let us derive this equation:

Given equations:

   P₄_{s} + 30₂_{g}  ⇒ P₄0₆_{s}  equation 1;

   P₄_{s} + 50₂_{g} ⇒  P₄0₁₀_{s}  equation 2;

To get the overall combined equation, the equation 1 must be reversed and added to equation 2:

            P₄0₆_{s} ⇒ P₄_{s} + 30₂_{g}   equation 3

                      +

            equation 2:

 P₄_{s} + 50₂_{g}  +    P₄0₆_{s}  ⇒  P₄0₁₀_{s}  +  P₄_{s} + 30₂_{g}  

cancelling specie that appears on both sides and removing excess oxygen gas on the reactant side gives;

   

                  P₄0₆_{s} + 20₂_{g}   ⇒    P₄0₁₀_{s}

learn more:

Net equation brainly.com/question/2947744

#learnwithBrainly

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Answer:

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Temperature change, colour change, releasing gas, bubbles and change in odor
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Given that the freezing point depression constant for water is 1.86°c kg/mol, calculate the change in freezing point for a 0.907
melamori03 [73]

Answer : The correct answer for change in freezing point = 1.69 ° C

Freezing point depression :

It is defined as depression in freezing point of solvent when volatile or non volatile solute is added .

SO when any solute is added freezing point of solution is less than freezing point of pure solvent . This depression in freezing point is directly proportional to molal concentration of solute .

It can be expressed as :

ΔTf = Freezing point of pure solvent - freezing point of solution = i* kf * m

Where : ΔTf = change in freezing point (°C)

i = Von't Hoff factor

kf =molal freezing point depression constant of solvent.\frac{^0 C}{m}

m = molality of solute (m or \frac{mol}{Kg} )

Given : kf = 1.86 \frac{^0 C*Kg}{mol}

m = 0.907 \frac{mol}{Kg} )

Von't Hoff factor for non volatile solute is always = 1 .Since the sugar is non volatile solute , so i = 1

Plugging value in expression :

ΔTf = 1* 1.86 \frac{^0 C*Kg}{mol} * 0.907\frac{mol}{Kg} )

ΔTf = 1.69 ° C

Hence change in freezing point = 1.69 °C

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3 years ago
Write the net ionic equation for the reaction that occurs when equal volumes of 0.546 M aqueous acetylsalicylic acid (aspirin) a
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Answer:

C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-

Explanation:

Hello there!

In this case, according to the given information, it turns out possible for us to figure out the required net ionic equation by firstly writing out the complete molecular equation between aspirin and sodium acetate:

C_9H_8O_4+NaC_2H_3O_2\rightarrow C_2H_4O_2+NaC_9H_7O_4

Whereas acetic acid and sodium acetylsalicylate are formed. Now, we write the complete ionic equation whereby sodium acetate and sodium acetylsalicylate are ionized because they are salts yet neither aspirin nor acetic acid are ionized as they are weak acids:

C_9H_8O_4+Na^++C_2H_3O_2^-\rightarrow C_2H_4O_2+Na^++C_9H_7O_4^-

Finally, for the net ionic equation we cancel out the sodium spectator ions to obtain:

C_9H_8O_4+C_2H_3O_2^-\rightarrow C_2H_4O_2+C_9H_7O_4^-

Regards!

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Explanation:

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