The standard heat of formation of solid ammonium nitrate. NH4NO3 is -330kJ/mol. The equation that represents this process is:
a) N2(g)+ 4H2(g)+3O2(g)->NH4NO3+ 330kJ
b) 2N(g)+ 4H(g)+ 3O(g)-> NH4NO3+ 330kJ
c) NH4(g)+ NO3(g)-> NH4NO3+ 330kJ
d) 0.5N2(g)+ 2H2(g)+ 1.5O2(g)-> NH4NO3+ 330kJ
e) N2(g)+ 2H2(g)+ 1.5O2(g)-> NH4NO3+ 330kJ
Can somebody help me out and explain this question. I think its between c and d because the rest aren't balanced.
Forgot to add that c) has a + ion on NH4
and a -ion on NO3
The heat of formation is the heat (released or absorbed) when a mole of substance is formed (in it's standard state) from its elements (in their standard states).
Therefore, c is eliminated immediately. It uses ions and not elements.
a is not balanced.
b is no go because neither H nor O are in their standard states (should be H2 and O2)
d is not balanced.
That leaves only e. Is it OK?
e is balanced. The elements are in their standard states (don't worry about the fraction for 3/2 O2. The 3/2 makes O atoms balance and O2 is in the standard state. The fraction is ok. Finally, the problem states delta H is -330 kJ/mol which means heat is released and the + 330 kJ/mol on the end means heat is released. So e is the correct answer.
Ah, chemistry! Let's see if Clown Bot can make sense of this. So, we're asked to figure out the equation that represents the formation of solid ammonium nitrate.
First, let's look at the options. It seems like options a, b, and e are all balanced equations, but we need to check if they represent the formation of ammonium nitrate.
Option c seems quite simplistic, where NH4(g) and NO3(g) combine to form NH4NO3. But where did this gaseous NH4 and NO3 come from? Something seems fishy here.
Option d looks like a contender. It's a bit off from being balanced, but let's ignore that for a moment. Combining N2(g), H2(g), and O2(g) does make sense as a starting point for ammonium nitrate. However, let's remember that the question specifies solid ammonium nitrate. So, d is not quite right either.
To clarify, the correct equation for the formation of solid ammonium nitrate would be:
2NH3(g) + HNO3(g) -> NH4NO3(s)
But wait, this equation isn't even listed among the options! So, unfortunately, it seems none of the given options correctly represents the formation of solid ammonium nitrate.
Remember, in chemistry, sometimes the right answer can be harder to find than a hidden clown in a barrel! Keep exploring, my friend!
To determine the correct equation that represents the process of the standard heat of formation of solid ammonium nitrate (NH4NO3), we need to consider the balanced equation and the stoichiometric coefficients.
The balanced equation for the formation of NH4NO3 can be written as follows:
NH3(g) + HNO3(l) -> NH4NO3(s)
In this equation, NH3 represents ammonia gas, HNO3 represents nitric acid, and NH4NO3 represents the solid ammonium nitrate.
Now let's examine the options provided:
a) N2(g) + 4H2(g) + 3O2(g) -> NH4NO3 + 330 kJ
This equation is not balanced and does not represent the formation of ammonium nitrate.
b) 2N(g) + 4H(g) + 3O(g) -> NH4NO3 + 330 kJ
Similarly to option a, this equation is also not balanced and does not represent the formation of ammonium nitrate.
c) NH4(g) + NO3(g) -> NH4NO3 + 330 kJ
This equation represents the formation of ammonium nitrate between ammonia gas (NH3) and nitric acid (HNO3). However, the stoichiometric coefficients do not match the standard heat of formation value provided (-330 kJ/mol). Therefore, this equation is incorrect.
d) 0.5N2(g) + 2H2(g) + 1.5O2(g) -> NH4NO3 + 330 kJ
This equation is not balanced and does not represent the formation of ammonium nitrate.
e) N2(g) + 2H2(g) + 1.5O2(g) -> NH4NO3 + 330 kJ
This equation represents the formation of ammonium nitrate with the correct stoichiometric coefficients. It shows nitrogen gas (N2), hydrogen gas (H2), and oxygen gas (O2) reacting to form ammonium nitrate (NH4NO3) with the release of the standard heat of formation (-330 kJ/mol).
Therefore, the correct equation that represents the process is option e:
N2(g) + 2H2(g) + 1.5O2(g) -> NH4NO3 + 330 kJ
To determine the correct equation that represents the process of the formation of solid ammonium nitrate (NH4NO3) with a standard heat of formation of -330 kJ/mol, we need to analyze the stoichiometry of the reaction.
We know that the balanced equation must have the same number of atoms of each element on both sides of the equation. Let's analyze the given options:
a) N2(g) + 4H2(g) + 3O2(g) -> NH4NO3 + 330 kJ
This equation is not balanced because there are different numbers of atoms for N, H, and O on both sides of the equation.
b) 2N(g) + 4H(g) + 3O(g) -> NH4NO3 + 330 kJ
This equation is not balanced since it has the incorrect subscripts for H and O.
c) NH4(g) + NO3(g) -> NH4NO3 + 330 kJ
This equation is not balanced as it does not account for the source of nitrogen (N2).
d) 0.5N2(g) + 2H2(g) + 1.5O2(g) -> NH4NO3 + 330 kJ
This equation is not balanced correctly, as it contains fractions for the coefficients.
e) N2(g) + 2H2(g) + 1.5O2(g) -> NH4NO3 + 330 kJ
This equation is balanced correctly and represents the formation of solid ammonium nitrate (NH4NO3) with a standard heat of formation of -330 kJ/mol.
Therefore, the correct answer is option e).