Since the question manages to include moles, pressure, volume, and temperature, then it is evident that in order to find the answer we will have to use the Ideal Gas Equation: PV = nRT (where P = pressure; V = volume; n = number of moles; R = the Universal Constant [0.082 L·atm/mol·K]; and temperature.
First, in order to work out the questions, there is a need to convert the volume to Litres and the temperature to Kelvin based on the equation: 250 mL = 0.250 L 58 °C = 331 K
Also, based on the equation P = nRT ÷ V
⇒ P = (2.48 mol)(0.082 L · atm/mol · K)(331 K) ÷ 0.250 L ⇒ P = (67.31 L · atm) ÷ 0.250 L ⇒ P = 269.25 atm
Thus the pressure exerted by the gas in the container is 269.25 atm.
what you have to do is to multiply the given grams with the ratio of grams of that certain element in it's full compound in order to isolate the compound and get the element.
because the question did not specify how many grams of NO2 is formed, we can assume that the mass is neglegible, thus 1 mole was assigned to Nitrogen.
