Question

A scientist plans the react 9.0x10^-2 L NO held at a pressure of 200.0kPa and a temperature of 20.0 C with excess hydrogen. How many moles of nitrogen gas will be produced

Answer 1

`n_(N_2)=0.00369molN_2`

Step-by-step explanation:

Hello there!

In this case, by firstly setting up the described chemical reaction, we are able to write:

`2NO(g)+2H_2(g)\rightarrow N_2(g)+2H_2O(g)`

Thus, given the pressure (convert to atm), volume and temperature (convert to K) we can calculate the moles of NO:

`n=(PV)/(RT)\\\\n=(200.00/101.325atm*0.090L)/(0.08206(atm*L)/(mol*K)*(20.0+273.15)K) \\\\n=0.00738molNO`

Next, we use the 2:1 mole ratio of NO to N2 to obtain the moles of nitrogen gas that will be produced:

`n_(N_2)=0.00738molNO *(1molN_2)/(2molNO) \\\\n_(N_2)=0.00369molN_2`

Regards!