A jar holds 2.0 L of ideal nitrogen gas, $\mathrm { N } _ { 2 }$ at STP. The atomic mass of nitrogen is 14.0 g/mol, the ideal gas constant is $R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K }$ Avogadro's number is $N _ { \mathrm { A } } = 6.022 \times$ $10^{23} \text { molecules/mol, }$ and 1.00 atm=101 kPa
(a) How many moles of nitrogen are in the jar?
(b) How many nitrogen molecules are in the jar?
(c) What is the mass of the nitrogen in the jar?

Question

A jar holds  2.0 L of ideal nitrogen gas, $\mathrm { N } _ { 2 }$ at STP. The atomic mass of nitrogen is  14.0 g/mol, the ideal gas constant is $R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K }$ Avogadro's number is $N _ { \mathrm { A } } = 6.022 \times$ $10^{23} \text { molecules/mol, }$ and  1.00 atm=101 kPa
(a) How many moles of nitrogen are in the jar?
(b) How many nitrogen molecules are in the jar?
(c) What is the mass of the nitrogen in the jar?

Quizplus · Accepted Answer

The Answer of A jar holds  2.0 L of ideal nitrogen gas, $\mathrm { N } _ { 2 }$ at STP. The atomic mass of nitrogen is  14.0 g/mol, the ideal gas constant is $R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K }$ Avogadro's number is $N _ { \mathrm { A } } = 6.022 \times$ $10^{23} \text { molecules/mol, }$ and  1.00 atm=101 kPa
(a) How many moles of nitrogen are in the jar?
(b) How many nitrogen molecules are in the jar?
(c) What is the mass of the nitrogen in the jar?

A Jar Holds 2 N2\mathrm { N } _ { 2 }N2​

A Jar Holds 2 $\mathrm { N } _ { 2 }$