if 37.9 liters of NO at .993atm and 146 degrees celcius are decomposed by the reaction 2NO-->N2+O2
how many grams of nitrogen will be formed...
could you show mw step bu step how to do this ? thanks....i have finals tommorrow.... i need HHHHHHEEEEEEELLLLLLPPPPPPPP
PV=nRT
P=0.993 atm
V = 37.9 L
n = solve for this
R = 0.080206 L*atm/mol*K
T = 273 + 146 = 419 Kelvin
n = 1.095 mols ofNO.
mols N2 formed from the reaction =
mols NO x (1 mol N2/2 mols NO)=
1.095 x 1/2 = 0.547
grams N2 = mols x molar mass which I will leave for you to do.
grams N2 = 0.547 x 28 = ??
Check my thinking. Check my arithmetic.
To calculate the number of grams of nitrogen (N2) formed from the given reaction, you can follow these steps:
Step 1: Calculate the number of moles of NO (nitric oxide) present in the initial condition using the ideal gas law equation, PV = nRT.
Given:
P (pressure) = 0.993 atm
V (volume) = 37.9 L
R (ideal gas constant) = 0.080206 L*atm/mol*K
T (temperature) = 419 K
Using the ideal gas law equation: PV = nRT
Substituting the given values:
(0.993 atm)(37.9 L) = n(0.080206 L*atm/mol*K)(419 K)
(n = (0.993 atm * 37.9 L) / (0.080206 L*atm/mol*K * 419 K))
n ≈ 1.095 moles of NO
Therefore, there are approximately 1.095 moles of NO in the initial condition.
Step 2: Calculate the number of moles of nitrogen (N2) formed from the reaction using the stoichiometry of the balanced equation.
Given:
2NO --> N2 + O2
From the balanced equation, it is clear that for every 2 moles of NO, 1 mole of N2 is formed.
Using the given information:
mols N2 formed from the reaction = mols NO x (1 mol N2 / 2 mol NO)
mols N2 = 1.095 moles x (1 mol N2 / 2 mol NO)
mols N2 ≈ 0.547 moles
Therefore, approximately 0.547 moles of nitrogen (N2) are formed from the reaction.
Step 3: Calculate the mass of nitrogen (N2) formed by multiplying the number of moles of nitrogen (N2) by its molar mass.
The molar mass of nitrogen (N2) is approximately 28 g/mol.
Using the given information:
grams N2 = mols N2 x molar mass
grams N2 = 0.547 moles x 28 g/mole
grams N2 ≈ 15.316 g
Therefore, approximately 15.316 grams of nitrogen (N2) will be formed from the given reaction.
It is important to double-check both the thinking process and the arithmetic to ensure accuracy. Good luck with your finals!