Answer:
2.23L
Explanation:
Using the general gas law as follows:
PV = nRT
Where;
P = pressure (atm)
V = volume (L)
n = number of moles (mol)
R = gas constant (0.0821 Latm/molK)
T = temperature (K)
According to the information provided in this question,
Mass of nitrogen = 2800mg
Since 1g = 1000mg
2800mg = 2800/1000
= 2.8g
Using mole = mass ÷ molar mass
Molar mass of nitrogen gas (N2) = 28g/mol
mole = 2.8/28
mole of N2 gas = 0.1mol
Pressure = 98kPa
1 kilopascal (kPa) = 1000pascal (pa)
98kPa = 98 × 1000
= 98000pascal
Since 1 Pascal = 9.869 × 10^-6 atmosphere (atm)
98000pascal = 98000 × 9.869 × 10^-6
= 0.967atm
Temperature = -10°C
Kelvin = °C + 273
Kelvin = -10 + 273
K = 263K
Hence, using PV = nRT
0.967 × V = 0.1 × 0.0821 × 263
0.967V = 2.159
V = 2.159/0.967
V = 2.23
Volume of Nitrogen gas = 2.23 L
