KS5 Ideal Gas Law

How many moles of gas are in a bike tire with a volume of 2.00 × 10⁻³ m³ , a pressure of 7.00 × 10⁵ Pa and at a temperature of 18.0ºC?

• 0.378

• 0.579

• 0.879

• 0.283

k = ?

• 8.31 × 10^–23 J/mol/K

• 1.38 × 10^–23 J/K/kg

• 6.023 × 10²³

• 1.38 × 10^–23 J/K

4.0 g of helium contains one mole. The helium is at a pressure of  $1.0\times10^5Pa$   and at a temperature of 300 K. What volume does is occupy?

• 0.025 cubic metres

• 0.15 cubic metres

• 0.039 cubic metres

• 0.52 cubic metres

Which of these is incorrect?

• $R=\frac{pV}{nT}$

• $k=\frac{pV}{NT}$

• $n=\frac{N_A.M_s}{M}$

• $k=\frac{pV}{nT}$

Boyles Law states that for a fixed mass of gas _________, then  $pV=constnt$  

One atomic mass unit is

• one twelfth of the mass of carbon - 12

• the number of atoms in 12g of carbon - 12

• the mass of one mole of a substance

• the number of atoms in 1g of hydrogen

What is the temperature of 19.0 m³ of an ideal gas at a pressure of 0.8 x 10⁵ Pa if the same gas occupies 12.0 m³ at 1.01 x 10⁵ Pa and 27^oC?

• 549K

• 762K

• 343K

• 285K

What would a graph of pV against T look like?

• A straight line through the origin.

• A curved line, asymptotic to both axis.

• A line of 0 gradient, intersecting at T = -273.15 degrees.

Are molar mass and molecular mass the same thing?

• Yes

• No

• Maybe

• I don't know

What is an expression for the Boltzmann constant?

• $k=\frac{N_A}{R}$

• $k=N.M_s$

• $k=\frac{R}{N_A}$

• $k=S\ln\Omega$