It’s blurry.... try again
Answer:
Mass of water = 73.08 g
Explanation:
Given data:
Mass of hydrogen = 35 g
Mass of oxygen = 65 g
Mass of water = ?
Solution:
First of all we will write the balanced chemical equation:
2H₂ + O₂ → 2H₂O
Number of moles of hydrogen = mass/ molar mass
Number of moles of hydrogen = 35 g/ 2 g/mol
Number of moles of hydrogen = 17.5 mol
Number of moles of oxygen = 65 g / 32 g/mol
Number of moles of oxygen = 2.03 moles
Now we compare the moles of water with moles hydrogen and oxygen.
H₂ : H₂O
2 : 2
17.5 : 17.5
O₂ : H₂O
1 : 2
2.03 : 2× 2.03 =4.06 mol
Number of moles of water produced by oxygen are less so oxygen is limitting reactant.
Mass of water:
Mass of water = number of moles × molar mass
Mass of water = 4.06 mol × 18 g/mol
Mass of water = 73.08 g
Answer:
Explanation:
The whole sample is 269
%copper = 127/269 * 100 = 47.2%
%chlorine = 142/269 * 100 = 52.8%
That's all you are asking. Is there more?
Answer:
1.8 x 10⁻⁵
Explanation:
NH3(aq) + H2O(l) ⇄ NH4⁺(aq) + OH⁻(aq)
I 0.95 0 0
C -x +x +x
E 0.95-x x x
Kb= [NH₄⁺] [OH⁻] / ( NH₃) = x²/ (0.95-x )
P(OH) = 14-PH = 14-11.612 = 2.388
(OH)⁻¹ = 10⁻²°³⁸⁸ = 4.09 x 10⁻³ = x
Kb = (4.09 x 10⁻³)²/ (0.95-4.09 x 10⁻³)
= 1.8 x 10⁻⁵
Answer:
Hope this helps
molar mass: 170.21 g/mol
Explanation:
If it did plzz mark brainliest
