Answer: 48.6 kJ/mol
Explanation:
The balanced chemical reaction is,
The expression for enthalpy change is,
where,
n = number of moles
(as heat of formation of substances in their standard state is zero
Now put all the given values in this expression, we get
Therefore, the enthalpy change for benzene is 48.6 kJ/mol
Answer:
The answer is 916.67 g
Explanation:
48.0 wt% NaOH means that there are 48 g of NaOH in 100 g of solution. With this information and the molecular weight of NaOH (40 g/mol), we can calculate the number of mol there are in 100 g of this solution:
x
= 0.012 mol NaOH/100 g solution
Finally, we need 0.11 mol in 1 liter of solution to obtain a 0.11 M NaOH solution.
0.012 mol NaOH ------------ 100 g solution
0.11 mol NaOH------------------------- X
X= 0.11 mol NaOH x 100 g/ 0.012 mol NaOH= 916.67 g
We have to weigh 916.67 g of 48.0%wt NaOH and dilute it in a final volume of 1 L of water to obtain a 0.11 M NaOH solution.
9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.
<h3>What is an ideal gas equation?</h3>The ideal gas law (PV = nRT) relates the macroscopic properties of ideal gases. An ideal gas is a gas in which the particles (a) do not attract or repel one another and (b) take up no space (have no volume).
Given data:
Oxygen produced - 1.618 gram
Decomposition of takes place.
Find - Amount of produced.
The decomposition reaction is as follows -
-->
Moles of gas =
=0.1 moles.
1 mole of is produced from 2 moles of dinitrogen pentoxide
0.1 mole of will be produced from = 0.2 moles.
Now, 2 moles of dinitrogen pentoxide produce 4 moles of
produced will be - 0.4 moles.
Weight of produced - 0.4 X 46
Weight of produced - 18.4 gram
Thus, grams of produced are 18.4
Now calculate the volume of
Given data are:
P=103.25 kPa =1.01899827 atm
T= 22.75 °C +273 = 295.75 K
n=0.4 moles
V=?
R= 0.0821 liter·atm/mol·K
Putting the value in PV=nRT
V =
V =
V= 9.5314 L
Hence, 9.5314 L is the volume of nitrogen dioxide formed at 103.25 kPa and 22.75 °C.
Learn more about the ideal gas equation here:
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