Answer:
Kp = 8.76×10⁻³
Explanation:
We determine the carbamate decomposition in equilibrium:
NH₄CO₂NH₂ (s) ⇄ 2NH₃(g) + CO₂(g)
Let's build the expression for Kp
Kp = (Partial pressure NH₃)² . Partial pressure CO₂
We do not consider, the carbamate because it is solid and we only need the partial pressure from gases
Kp = (0.370atm)² . 0.0640 atm
Kp = 8.76×10⁻³
Remember Kp does not carry units
like this variable variable variable variable
Answer: The molarity of the borax solution is 0.107 M
Explanation:
The neutralization reaction is:
According to neutralization law:
where,
= basicity of 
= 2
= acidity of borax = 2
= concentration of = 1.03 M
= concentration of borax =?
= volume of = 2.07ml
= volume of borax = 20.0 ml
Now put all the given values in the above law, we get the molarity of borax:
By solving the terms, we get :
Thus the molarity of the borax solution is 0.107 M
<span>Balanced equation:
2 CU(NO3)2 = 2 CUO + 4 NO2 + O2</span>
<span>Reaction type: decomposition</span>
The balanced equation for the reaction between Ba(OH)₂ and HCl is as follows;
Ba(OH)₂ + 2HCl ---> BaCl₂ + 2H₂O
stoichiometry of Ba(OH)₂ to HCl is 1:2
the number of HCl moles that have reacted - 0.2452 mol/L x (20.00 x 10⁻³ L)
number of HCl moles reacted = 0.004904 mol
2 mol of HCl reacts with 1 mol of Ba(OH)₂
therefore 0.004904 mol of HCl reacts with - 1/2 x 0.004904 mol of Ba(OH)₂
number of Ba(OH)₂ moles in 18.15 mL - 0.002452 mol
Therefore number of Ba(OH)₂ moles in 1000 mL- 0.002452 mol /(18.15 x 10⁻³ L)
molarity of Ba(OH)₂ is = 0.1351 M
