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3 years ago

Select the correct answer.

Chemistry

1 answer:

Norma-Jean [14]3 years ago

7 0

Answer:

a t o m i c w e i h g t

Explanation:

a to m i c w e i g h t

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15. Ammonium nitrate, NH4NO3, and aluminum powder react explosively producing nitrogen gas, water vapor and aluminum oxide. Writ

Lunna [17]

Answer:

$2Al_(_S_) ~+~3NH_4NO_3_(_a_q_) ->3N_2_(_g_) ~+~6H_2O_(_g_) ~+~Al_2O_3_(_S_)$

$Entalpy=-2861.9~KJ$

Explanation:

In this case, we have to start with the reagents:

$Al~+~NH_4NO_3$

The compounds given by the problem are:

-) Nitrogen gas = $N_2$

-) Water vapor = $H_2O$

-) Aluminum oxide = $Al_2O_3$

Now, we can put the products in the reaction:

$Al_(_S_) ~+~NH_4NO_3_(_aq_) ->N_2_(_g_) ~+~H_2O_(_g_) ~+~Al_2O_3_(_S_)$

When we balance the reaction we will obtain:

$2Al_(_S_) ~+~3NH_4NO_3_(_a_q_) ->3N_2_(_g_) ~+~6H_2O_(_g_) ~+~Al_2O_3_(_S_)$

Now, for the enthalpy change, we have to find the standard enthalpy values:

$Al_(_S_)=0~KJ/mol$

$NH_4NO_3_(_a_q_)=-132.0~KJ/mol$

$N_2_(_g_)=0~KJ/mol$

$H_2O_(_g_)=~-~241.8~KJ/mol$

$Al_2O_3_(_S_)=~-~1675.7~KJ/mol$

With this in mind, if we multiply the number of moles (in the balanced reaction) by the standard enthalpy value, we can calculate the energy of the reagents:

$(0*2)~+~(-132*3)=~-396~KJ$

And the products:

$(0*3)~+~(-241.8*6)~+~(-1675.7*1)=-3125.9~KJ$

Finally, for the total enthalpy we have to subtract products by reagents :

$(-3125.9~KJ)-(-396~KJ)=-2729.9~KJ$

I hope it helps!

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pshichka [43]

Answer:

extensive

hope it helps!

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