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2 years ago

We bored Meeting id:333-065-2087 Password:5FRgXJ

Chemistry

2 answers:

MAXImum [283]2 years ago

7 0

BET
I'll join never.
Stop posting stuff other than questions.

Juli2301 [7.4K]2 years ago

4 0

Answer:

pls don't post irrelevant questions

Explanation:

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How to know if a single replacement reaction will occur

Lerok [7]

Answer:

To determine whether a given single replacement will occur, you must use an “Activity Series” table. If the metal or the halogen is above the element it will replace based on the activity series, a single displacement reaction will occur. The video below summarizes an experiment conducted to compare the activities of three metals ( Mg, Cu and Zn ).

Explanation:

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2 years ago

.The chemical formula for table sugar is C12H11022. What can you tell from this formula?

34kurt

Answer:

The answer is: The ratio of oxygen atoms to hydrogen atoms in a molecule of sugar is 2 to 1.

Let me know if you need any other help:))

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3 years ago

Name the following ionic compound KBr

Semenov [28]

Potassium bromide found it on google

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3 years ago

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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3 years ago

What is the pressure in atmospheres exerted by a 0.500 mole sample of nitrogen gas in a 10.0 L

Nonamiya [84]

Answer:

The pressure is 1, 22 atm.

Explanation:

We use deal gas formula. First, we convert the unit of temperature in Celsius into Kelvin. We use the constant R= 0,082 l atm /K mol.Then, we solve P (pressure).

0°C=273 K 25°C= 273 + 25= 298 K

PV=nRT -----> P= (nRT)/V

P= (0,5 mol x 0,082 l atm /K mol x 298 K)/ 10 L

P= 1, 2218 atm

3 0

3 years ago