Question

At 40.0°C, the pressure inside a nitrogen-filled tennis ball with a volume of 148

Answer 1

Answer : The correct option is, (B) $1.34\times 10^2mol$

Explanation :

To calculate the moles of nitrogen gas we are using ideal gas equation:

$PV=nRT$

where,

P = pressure of nitrogen gas = 235 kPa = 2.319 atm

Conversion used : (1 atm = 101.325 kPa)

V = volume of nitrogen gas = $148cm^3=148mL=0.148L$

Conversion used : (1 L= 1000 mL)

T = temperature of nitrogen gas = $40.0^oC=273+40.0=313K$

R = gas constant = 0.0821 L.atm/mole.K

n = moles of nitrogen gas = ?

Now put all the given values in the ideal gas equation, we get:

$(2.319atm)\times (0.148L)=n\times (0.0821L.atm/mole.K)\times (313K)$

$n=0.0134mol=1.34\times 10^2mol$

Therefore, the number of moles of nitrogen gas are, $1.34\times 10^2mol$

Answer 2

Answer:

the answer is

n = 0.01336 mol

Explanation:

To determine the number of moles of a gas, we need to have an expression that relates the pressure, temperature and volume of the system. For simplification, we assume that this gas is ideal so we use the equation PV=nRT. We calculate as follows:

PV=nRT

n = PV / RT

n = 235000(1.48x10^-4) / (8.314)(40+273.15)

n = 0.01336 mol