A sealed container holds 0.020 moles of ideal nitrogen $\left( \mathrm { N } _ { 2 } \right)$ gas, at a pressure of 1.5 atm and a temperature of 290 K. The atomic mass of nitrogen is 14.0 g/mol. How many molecules of nitrogen are in the container? $( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1 \mathrm {~atm} = 101 \mathrm { kPa } )$
A) $6.0 \times 10 ^ { 21 } \mathrm {~mol}$
B) $2.4 \times 10^{22} \mathrm {~mol}$
C) $1.2 \times 10 ^ { 22 } \mathrm {~mol}$
D) $3.0 \times 10 ^ { 21 } \mathrm {~mol}$
E) $1.5 \times 10^{21} \mathrm {~mol}$

Question

A sealed container holds  0.020  moles of ideal nitrogen $\left( \mathrm { N } _ { 2 } \right)$ gas, at a pressure of  1.5 atm and a temperature of  290 K. The atomic mass of nitrogen is  14.0 g/mol. How many molecules of nitrogen are in the container? $( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1 \mathrm {~atm} = 101 \mathrm { kPa } )$
A) $6.0 \times 10 ^ { 21 } \mathrm {~mol}$
B) $2.4 \times 10^{22} \mathrm {~mol}$
C) $1.2 \times 10 ^ { 22 } \mathrm {~mol}$
D) $3.0 \times 10 ^ { 21 } \mathrm {~mol}$
E) $1.5 \times 10^{21} \mathrm {~mol}$

Quizplus · Accepted Answer

The number of molecules is calculated using Avogadro's number: $0.020 \, \text{moles} \times 6.022 \times 10^{23} \, \text{molecules/mole} = 1.2 \times 10^{22} \, \text{molecules}$.

A Sealed Container Holds 0 (N2)\left( \mathrm { N } _ { 2 } \right)(N2​)

A Sealed Container Holds 0 $\left( \mathrm { N } _ { 2 } \right)$