Respuesta :
To answer this question we have to usethe ideal gas law:
[tex]PV=nRT[/tex]Where P is the pressure, V is the volume, n is the number of moles, R is the constant of ideal gases (0.082atmL/molK) and T is the temperature (in Kelvin degrees).
The first step is to convert the given mass of N2 to moles using its molecular mass:
[tex]26.5gN_2\cdot\frac{molN_2}{28gN_2}=0.95molN_2[/tex]And convert the pressure from mmHg to atm (1atm=760mmHg):
[tex]640mmHg\cdot\frac{1atm}{760mmHg}=0.84atm[/tex]Finally, solve the initial equation for T and replace for the given values:
[tex]\begin{gathered} T=\frac{PV}{nR} \\ T=\frac{0.84atm\cdot50.0L}{0.95mol\cdot0.082atmL/molK} \\ T=539.15K \end{gathered}[/tex]The temperature of the gas is 539.15K.
Convert this temperature to Celsius by substracting 273.15 to the temperature in Kelvins:
[tex]T=539.15-273.15=226[/tex]The temperature of the gas is 226°C.
