Answer: There are [tex]4.45\times 10^{-4}moles[/tex] of gas are in a container with a volume of 9.55 mL at 35 °C and a pressure of 895 mmHg
Explanation:
According to ideal gas equation:
[tex]PV=nRT[/tex]
P = pressure of gas = 895 mm Hg= 1.18 atm (760 mm Hg= 1 atm)
V = Volume of gas = 9.55 ml = 0.00955 L (1 L=1000ml)
n = number of moles = ?
R = gas constant =[tex]0.0821Latm/Kmol[/tex]
T =temperature =[tex]35^0C=(35+273)K=308K[/tex]
[tex]n=\frac{PV}{RT}[/tex]
[tex]n=\frac{1.18atm\times 0.00955L}{0.0821L atm/K mol\times 308K}=4.46\times 10^{-4}moles[/tex]
Thus there are [tex]4.45\times 10^{-4}moles[/tex] of gas are in a container with a volume of 9.55 mL at 35 °C and a pressure of 895 mmHg
