Answer:
NaCl + AgF → NaF + AgCl
Explanation:
A double replacement reaction is a type of chemical reaction that occurs when two reactants exchange cations or anions to yield two new products.
From all the reactions given ,
- 2Na + Cl₂ → 2NaCl is an example of combination reaction because two or more reactants (Na & Cl₂) react with each other to form a single product (NaCl)
- H₂SO₃ → H₂O + SO₂ is an example of decomposition reaction because a single reactant (H₂SO₃) breaks down into two or more products (H₂O & SO₂).
- 2K + 2H₂O → 2KOH + H₂ is an example of displacement reaction because a highly reactive element (K) displaces a least reactive element (H) from its compound (H₂O).
- NaCl + AgF → NaF + AgCl is an example of double replacement reaction because there's an exchange between Cations (
& 
) and Anions (
& 
).
Because they are closer to the farther end of the periodic table. Since they are closer to the farther end they don't want to give away their electrons because it would be easier for them to just steal them from other atoms.
Answer:
1.784 g
Explanation:
The equation of the reaction is;
NaOH(aq) + KHC8H4O4(aq) --------> KNaC8H4O4(aq) + H2O(l)
Number of moles of NaOH reacted = 17.47/1000 * 0.5000 M
Number of moles of NaOH reacted =8.735 * 10^-3 moles
From the reaction equation;
1 mole of NaOH reacted with 1 mole of KHC8H4O4
Hence, 8.735 * 10^-3 moles of NaOH reacts with 8.735 * 10^-3 moles of KHP.
So,
Mass of KHP reacted = 8.735 * 10^-3 moles * 204.2 g/mol = 1.784 g
Answer:
Explanation:
In the solution of AB , they are split to give ions as follows
AB ⇄ A⁺ + B⁻
Product of concentration of A⁺ and B⁻ in saturated solution of AB is constant .
This is called Ksp
Ksp = [A⁺] [ B⁻]
If product of concentration of A⁺ and B⁻ exceeds Ksp , the equilibrium shifts to the left side and excess ions come out of solution in the form of precipitate. So second option is the answer.
Answer:
Answer:
step 1:balance skeleton equation the chemical equation:
Zn +HNO3➔Zn(NO3)2+NO+H2O
step 2: identity undergoing oxidation or reduction
here
Zn➔Zn(NO3)2
Zn is oxidized from 0 to 2 in oxidation no.
HNO3➔NO
N is reduced from 5 to 2 in oxidation no
Step 3: calculate change in oxidation no.
change in oxidation no
in Zn=0-2=-2=2
in
N=5-2=3
Step 4: Balance it by doing crisscrossed multiplication
we get;
3Zn +2HNO3➔3Zn(NO3)2+2NO+H2O
step 6:Balance other atoms except H & O
3Zn +2HNO3➔3Zn(NO3)2+2NO+H2O
3Zn +2HNO3+6HNO3➔3Zn(NO3)2+2NO+H2O
finally: balance H
<em><u>3Zn +8HNO3➔3Zn(NO3)2+2NO+4H2O</u></em>
