A $0.40 - \mathrm { m } ^ { 3 }$ gas tank holds 7.0 moles of ideal diatomic nitrogen gas at a temperature of 290 K. The atomic mass of nitrogen is 14.0 g/mol. What is the pressure of the gas? $( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1 \mathrm {~atm} =$ $101 \text { kPa) }$
A) 37 atm
B) 22 atm
C) 42 atm
D) 32 atm
E) 27 atm

Question

A $0.40 - \mathrm { m } ^ { 3 }$ gas tank holds  7.0  moles of ideal diatomic nitrogen gas at a temperature of  290 K. The atomic mass of nitrogen is  14.0 g/mol. What is the pressure of the gas? $( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1 \mathrm {~atm} =$ $101 \text { kPa) }$
A)  37 atm
B)  22 atm
C)  42 atm
D)  32 atm
E)  27 atm

Quizplus · Accepted Answer

The Answer of A $0.40 - \mathrm { m } ^ { 3 }$ gas tank holds  7.0  moles of ideal diatomic nitrogen gas at a temperature of  290 K. The atomic mass of nitrogen is  14.0 g/mol. What is the pressure of the gas? $( R = 8.31 \mathrm {~J} / \mathrm { mol } \cdot \mathrm { K } , 1 \mathrm {~atm} =$ $101 \text { kPa) }$
A)  37 atm
B)  22 atm
C)  42 atm
D)  32 atm
E)  27 atm

A 0.40−m30.40 - \mathrm { m } ^ { 3 }0.40−m3

A $0.40 - \mathrm { m } ^ { 3 }$