Answer:
Explanation:1. A 2.650-g sample of a gas occupies a volume of 428 mL at 0.9767 atm and 297.3 K. What is its molar mass?
2.
a. A sample of nitrogen gas has a volume of 10.0 L at 2.50atm and 50.0℃. If the pressure is increased to 5.00 atm and the temperature decreases to 25.0℃, what volume does the gas occupy?
(a). 5.00L, (b).4.61L, (c).2.50L, (d).5.42L
b. Using the average bond energy, calculate the enthalpy of the above reaction. draw Lewis structures of the reactants and products first to determine the exact bond order. N2(g)+3H2(g)→2NH3(g)
Given values are:
As we know the relation,
→ [tex]PV = nRT[/tex]
or,
→ [tex]n = \frac{PV}{RT}[/tex]
By substituting the values, we get
[tex]= \frac{0.9767\times 0.428}{0.0821\times 297.3}[/tex]
[tex]= 0.0171 \ moles[/tex]
hence,
The molar mass will be:
= [tex]\frac{Mass \ of \ gas}{Number \ of \ moles}[/tex]
= [tex]\frac{2.65}{0.0171}[/tex]
= [tex]155 \ g/mol[/tex]
Thus the above answer is right.
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