Answer:
The heat produced is -15,1kJ
Explanation:
For the reaction:
2SO₂+O₂ → 2SO₃
The enthalpy of reaction is:
ΔHr = 2ΔHf SO₃ - 2ΔHf SO₂
As ΔHf SO₃ = -395,7kJ and ΔHf SO₂ = -296,8kJ
<em>ΔHr = -197,8kJ</em>
Using n=PV/RT, the moles of reaction are:
= <em>0,153 moles of reaction</em>
As 2 moles of reaction produce -197,8kJ of heat, 0,153moles produce:
0,153mol× = <em>-15,1kJ</em>
<em></em>
I hope it helps!
Answer:
Explanation:
You need to remember that the oxidation number of H is +1, except when it is in a metal hydrites like NaH, where its oxidation number is -1. Then, the oxidation number of O is -2, but in peroxides is -1. So with these rules you just have to multiply the ox. number with the name of atoms and all the elements in the reaction must sum 0.
Answer:
<h3>1)</h3>Structure One:
Structure Two:
Structure Three:
Structure Number Two would likely be the most stable structure.
<h3>2)</h3>The N atom is the one that is "likely" to be attracted to an anion. See explanation.
Explanation:
When calculating the formal charge for an atom, the assumption is that electrons in a chemical bond are shared equally between the two bonding atoms. The formula for the formal charge of an atom can be written as:
.
For example, for the N atom in structure one of the first question,
The formal charge of this N atom will be .
Apply this rule to the other atoms. Note that a double bond counts as two bonds while a triple bond counts as three.
<h3>1)</h3>Structure One:
Structure Two:
Structure Three:
In general, the formal charge on all atoms in a molecule or an ion shall be as close to zero as possible. That rules out Structure number one.
Additionally, if there is a negative charge on one of the atoms, that atom shall preferably be the most electronegative one in the entire molecule. O is more electronegative than N. Structure two will likely be favored over structure three.
<h3>2)</h3>Similarly,
Assuming that electrons in a chemical bond are shared equally (which is likely not the case,) the nitrogen atom in this molecule will carry a positive charge. By that assumption, it would attract an anion.
Note that in reality this assumption seldom holds. In this ion, the N-H bond is highly polarized such that the partial positive charge is mostly located on the H atom bonded to the N atom. This example shows how the formal charge assumption might give misleading information. However, for the sake of this particular problem, the N atom is the one that is "likely" to be attracted to an anion.
Answer : The volume of reactant measured at STP left over is 409.9 L
Explanation :
First we have to calculate the moles of and
by using ideal gas equation.
<u>For :</u>
where,
P = Pressure of gas at STP = 1 atm
V = Volume of gas = 1580 L
n = number of moles = ?
R = Gas constant =
T = Temperature of gas at STP = 273 K
Putting values in above equation, we get:
<u>For :</u>
where,
P = Pressure of gas at STP = 1 atm
V = Volume of gas = 3510 L
n = number of moles = ?
R = Gas constant =
T = Temperature of gas at STP = 273 K
Putting values in above equation, we get:
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 3 mole of react with 1 mole of
So, 156.6 moles of react with
moles of
From this we conclude that, is an excess reagent because the given moles are greater than the required moles and
is a limiting reagent and it limits the formation of product.
Now we have to calculate the excess moles of reactant (unreacted gas).
Excess moles of reactant = 70.49 - 52.2 = 18.29 moles
Now we have to calculate the volume of reactant, measured at STP, is left over.
where,
P = Pressure of gas at STP = 1 atm
V = Volume of gas = ?
n = number of moles of unreacted gas = 18.29 moles
R = Gas constant =
T = Temperature of gas at STP = 273 K
Putting values in above equation, we get:
Therefore, the volume of reactant measured at STP left over is 409.9 L