Answer:
Kc for this reaction is 0.43
Explanation:
This is the equilibrium:
N₂(g) + 2H₂O(g) → 2NO(g) +2H₂(g)
And we have all the concentration at equilibrium:
N₂: 0.25M
H₂ : 1.3M
NO: 0.33M
H₂: 1.2M
They are ok, because they are in MOLARITY. (mol/L)
Let's make the expression for Kc
Kc = ( [NO]² . [H₂]² ) / ([N₂] . [H₂O]²)
Kc = (0.33² . 1.2²) / (0.25 . 1.2²)
Kc = 0.4356
In two significant digits. 0.43
Answer:
6.00%
Explanation:
Step 1: Given data
Accepted value for the number of calories in a Bananas Foster: 300 calories
Measured value for the number of calories in a Bananas Foster: 318 calories
Step 2: Calculate the percent error in the measure
We will use the following expression.
%error = |accepted value - experimental value|/ accepted value × 100%
%error = |300 cal - 318 cal|/ 300 cal × 100% = 6.00%
I think your answer is A not sure tho
Answer:
Option 4 with o-h in the most polar bond, since the two atoms in the bond have the greatest difference in electronegativity. This is assuming there are no other factors in other atoms bound to either of the elements in the bond.
Explanation:
