Question

Figure 13.8 shows plot of PV/T versus Pfor 1.00×10–3 kg of oxygen gas at two different temperatures.



(a) What does the dotted plot signify?

(b) Which is true: T1 > T2 or T1 < T2?

(c) What is the value of PV/T where the curves meet on the y-axis?

(d) If we obtained similar plots for 1.00 ×10–3 kg of hydrogen, would we get the same value of PV/T at the point where the curves meet on the y-axis? If not, what mass of hydrogen yields the same value of PV/T (for low pressure high temperature region of the plot)? (Molecular mass of H2 = 2.02 u, of O2 = 32.0 u, R = 8.31 J mo1–1 K–1.)

Answer 1

(a) dotted plot is parallel to X - axis , signifying that nR [ PV/T = nR ] is independent of P . hence it is representing ideal gas behavior .

(b) the graph at temperature T1 is closer to ideal behaviour ( becoz closer to dotted line ) hence, T1 > T2 . ( higher the temperatures , ideal behaviour is the higher ) .

(c) use PV = nRT
PV/T = nR
Mass of the gas = 1 × 10^-3 kg = 1 g
Molecular mass of O2 = 32g/mol
So, number of mole = given weight/molecular weight
= 1/32
So, nR = 1/32 × 8.314 = 0.26 J/K
Hence, value of PV/T = 0.26 J/K

(d) 1 g of H2 doesn't represent the same number of mole . e.g molecular mass of H2 = 2g/mol
Hence, number of miles of H2 require is 1/32 ( A/C to question , )
So, mass of H2 required = no of mole of H2 × molecular mass of H2
= 1/32 × 2
= 1/16 g

Answer 2

hope this helps ! have a good day !