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Arada [10]
3 years ago
14

Balance the equation and identify the type of reaction for ? P4(s) + ? Ca(s) → ? Ca3P2(s). 1. 2; 6; 2 — decomposition 2. 2; 6; 2

— displacement 3. 1; 6; 2 — displacement 4. 1; 6; 2 — synthesis 5. 2; 6; 2 — synthesis 6. 1; 6; 2 — decomposition
Chemistry
1 answer:
pishuonlain [190]3 years ago
5 0

Answer:

4. 1; 6; 2 — synthesis

Explanation:

<u>Decomposition reaction </u>is defined as the reaction in which a single large substance breaks down into two or more smaller substances.

AB\rightarrow A+B

<u>Single displacement </u>reaction is defined as the reaction in which more reactive element displaces a less reactive element from its chemical reaction.

The reactivity of metal is determined by a series known as reactivity series. The metals lying above in the series are more reactive than the metals which lie below in the series.

A+BC\rightarrow AC+B

<u>Synthesis reaction</u> is defined as the reaction in which smaller substances combine in their elemental state to form a larger substance.

A+B\rightarrow AB

The unbalanced combustion reaction is shown below as:-

P_4+Ca\rightarrow Ca_3P_2

On the left hand side,  

There are 4 phosphorus atoms and 1 calcium atom

On the right hand side,  

There are 2 phosphorus atoms and 3 calcium atoms

Thus,  

Right side, Ca_3P_2 must be multiplied by 2 to balance phosphorus.

Left side, Ca is multiplied by 6 so to balance the whole reaction.

Thus, the balanced reaction is:-

P_4+6Ca\rightarrow 2Ca_3P_2

Thus, answer:- 4. 1; 6; 2 — synthesis

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Calculate the enthalpy change, ∆H in kJ, for the reaction H2O(s) → H2(g) + 1/2O2(g). Use the following information: : +279.9 kJ
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Answer:

+ 291.9 kJ

Solution:

The equation given is as;

H₂O ₍s₎ → H₂ ₍g₎ + 1/2 O₂ ₍g₎ ΔH = ?

First, as we know the heat of formation of H₂O ₍l₎ is,

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Now, adding last two equations,

H₂O ₍l₎ → H₂ ₍g₎ + 1/2 O₂ ₍g₎ ΔH = + 285.9 kJ

H₂O ₍s₎ → H₂O ₍l) ΔH = + 6.0 kJ

-----------------------------------------------------------------------------

H₂O ₍s₎ → H₂ ₍g₎ + 1/2 O₂ ₍g₎ ΔH = + 291.9 kJ

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