Answer:
1.42 Kg of NaHCO3
Explanation:
From
Co= 10 pd/M
Where;
Co= concentration of the stock solution of acid
p= percentage of raw acid = 36%
d= density of the acid= 1.138g/mL
M= molar mass of the acid= 36.5 g/mol
Co= 10 × 36 × 1.138/36.5
Co= 11.22 M
Number of moles of acid= CV = 11.22 M × 1.508 L= 16.9 moles
The reaction equation is;
NaHCO3(aq)+HCl(aq)→NaCl(aq)+H2O(l)+CO2(g)
If 1 mole of NaHCO3 reacts with 1 mole of HCl
Then 16.9 moles of HCl reacts with 16.9 moles of NaHCO3
Hence 16.9 moles of NaHCO3 is required to neutralize the HCl.
From
n= m/ M
Where;
n= number of moles = 16.9
m= mass of NaHCO3= ??
M= molar mass of NaHCO3= 84.007 g/mol
m= n× M/1000
m= 16.9 × 84.007 /1000
m= 1.42 Kg
More context to this question?
Answer:
B. All people on the night side of Earth
Explanation:
A lunar eclipse is a phenomenon that occurs when the Earth comes between the Moon and the Sun thereby causing it to cover the Moon with its shadow.
Simply stated, lunar eclipse takes place when the Moon passes or moves through the Earth's shadow thereby blocking any ray of sunlight from reaching the Moon. Thus, the full moon appears deep red (blood moon).
Also, a lunar eclipse would occur only when the Sun, Earth, and Moon are closely aligned to form a straight line known as the syzygy.
There are three (3) types of lunar eclipse and these are;
1. Total lunar eclipse.
2. Partial lunar eclipse.
3. Penumbra lunar eclipse.
<em>In a nutshell, all people on the night side of Earth can witness a lunar eclipse and have a good view of the Moon. </em>
Mass percent of methanol :
% mass = mass methanol / mass total
% mass = 15.0 / 100.0 + 10.0 + 15.0
% mass = 15.0 / 125.0
% mass ( methanol ) = 0,12 x 100 = 12%
hope this helps!
Answer is: 2Zn + O₂ → 2ZnO (2Zn²⁺ + 2O²⁻).
Unbalanced chemical reaction: Zn + O₂ → ZnO.
Zn → Zn²⁺ + 2e⁻ / ×2; 2Zn → 2Zn²⁺ + 4e⁻.
4e⁻ + O₂ → 2O²⁻.
Zinc lost two electrons and became Zn²⁺, molecule of oxygen gain four electrons and become 2O²⁻. Multiply first reaction with two to have same number of electrons and put coefficients in chemical reaction.
