Answer:
1223.38 mmHg
Explanation:
Using ideal gas equation as:

where,  
P is the pressure
V is the volume
n is the number of moles
T is the temperature  
R is Gas constant having value = 
Also,  
Moles = mass (m) / Molar mass (M)
Density (d)  = Mass (m) / Volume (V)
So, the ideal gas equation can be written as:

Given that:- 
d = 1.80 g/L
Temperature = 32 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15  
So,  
T = (32 + 273.15) K = 305.15 K 
Molar mass of nitrogen gas = 28 g/mol
Applying the equation as:
P × 28 g/mol  = 1.80 g/L × 62.3637 L.mmHg/K.mol × 305.15 K 
⇒P = 1223.38 mmHg
<u>1223.38 mmHg must be the pressure of the nitrogen gas.</u>
 
        
             
        
        
        
Answer:
there are four peaks in the 13c NMR (B)
 
        
             
        
        
        
Answer:
1)Reactants
2)Light
3)An item that can increase reaction rates
4)Reactants must collide with each other
Less molecules lower the chance for collisions
The more collisions there are the higher the reaction rate