Balance the equation.
N2 + 3Cl2 ==> 2NXl3 dH = 230 kJ
If 28g N2 absorbs 230 kJ, then how much N2 is needed to absorb only 96.5?
28 x (96.5/230) = ?
Convert g N2 from part a to mols. mol grams/molar mass = ?
Use the coefficients in the balanced equation to convert mols N2 to mols Cl2.
Then mols Cl2 x 22.4 L/mol = L Cl2 at STP
Given the following equation:
N2 + Cl2 > @ NCL3 H=+230 kJ
a) What mass of N2 would absorb 96.5 kJ of heat as it reacts?
b) What volume of Cl2 at STP would be required to react with the N2 in part (a)?
I do not know how to solve this problem. My mindset is that it involves stoichiometry in some way, I do not know how to manipulate it though.
4 answers
I got 11.8 for A
and 14.15 for B
and 14.15 for B
I obtained 11.7 for A. You probably used 14.008 for N.
The only way I can get your answer to part B is to convert mols N2 as 11.8/14 but it should be 11.8/28 = mols N2 = 0.421.
Then 0.421 x (3 mols Cl2/1 mol N2) = mols Cl2.
mols Cl2 x 22.4 = about 28.3 L
The only way I can get your answer to part B is to convert mols N2 as 11.8/14 but it should be 11.8/28 = mols N2 = 0.421.
Then 0.421 x (3 mols Cl2/1 mol N2) = mols Cl2.
mols Cl2 x 22.4 = about 28.3 L
AHH! I accidentally put 2 mols for N2 instead of 1 I see now
2 answers