What is the pressure of NO gas (density 1.34 g/L) at 25 $\circ$ C?

Question

Quizplus · Accepted Answer

First, we need to convert the temperature to Kelvin:
25°C + 273.15 = 298.15 K
Then, we can use the ideal gas law: PV = nRT
where P is pressure (in atm), V is volume (in L), n is the number of moles, R is the gas constant (0.08206 L·atm/(mol·K)), and T is temperature (in K).
We can find n by dividing the density by the molar mass of NO gas: 
1.34 g/L ÷ 30.01 g/mol = 0.0447 mol/L
Now we can rearrange the ideal gas law equation to solve for P:
P = nRT / V
P = (0.0447 mol/L) x (0.08206 L·atm/(mol·K)) x (298.15 K) / 1 L
P = 1.09 atm (rounded to two significant figures)

What Is the Pressure of NO Gas (Density 1 ∘\circ∘ C? A)0

What Is the Pressure of NO Gas (Density 1 $\circ$ C?
A)0