Answer:
They are in this position
Identify the precipitation reactions. drag the appropriate items to their respective bins.
2 answers:
The precipitation reactions :
2KBr + Pb(NO₃)₂ -----> PbBr₂ + 2KNO₃
Hg₂(C₂H₃O₂)₂ + 2NaI ----> Hg₂I₂ + 2NaC₂H₃O₂
Ba(NO₃)₂ + K₂SO₄ -----> BaSO₄ + 2KNO₃
<h3>Further explanation </h3>There are two types of chemical reactions that may occur,
namely single-replacement reactions and double-replacement reactions.
1. A single replacement reaction is a chemical reaction in which one element replaces the other elements of a compound to produce new elements and compounds
Not all of these reactions can occur. We can use the activity series, which is a list of elements that can replace other elements below / to the right of them in a single replacement reaction.
2. Double-Replacement reactions. Happens if there is an ion exchange between two ion compounds in the reactant to form two new ion compounds in the product
To predict whether this reaction can occur or not is to see the precipitation reaction. A precipitation reaction occurs if two ionic compounds which are dissolved reacted to produce one of the products of the ion compound does not dissolve. Formation of these precipitating compounds that cause reactions can occur
Solubility Rules:
- 1. soluble compound
All compounds of Li +, Na +, K +, Rb +, Cs +, and NH4 +
All compounds of NO₃⁻ and C₂H₃O₂⁻
Compounds of Cl−, Br−, I− except Ag⁺, Hg₂²⁺, Pb²⁺
Compounds of SO₄²⁻ except Hg₂²⁺, Pb²⁺, Sr²⁺, Ba²⁺
- 2. insoluble compounds
Compounds of CO₃²⁻ and PO₄³⁻ except for Compounds of Li +, Na +, K +, Rb +, Cs +, and NH₄ +
Compounds of OH− except Compounds of Li +, Na +, K +, Rb +, Cs +, NH₄⁺, Sr²⁺, and Ba²⁺
Let's look at possible reactions that are not shown in the question
1. S + O₂ ---> SO₂
SO₂ = gas so this reaction not the precipitation reactions
2. H₂O₂ + NaIO ---> NaI + H₂O + O₂
NaI = soluble so this reaction not the precipitation reactions
3. 2KBr + Pb(NO₃)₂ -----> PbBr₂ + 2KNO₃
PbBr₂ precipitates = so this reaction the precipitation reactions
4. HCl + KOH ----> KCl + H₂O
KCl soluble so this reaction not the precipitation reactions
5. HBr + KOH ----> KBr + H₂O
KBr soluble so this reaction not the precipitation reactions
6. Hg₂(C₂H₃O₂)₂ + 2NaI ----> Hg₂I₂ + 2NaC₂H₃O₂
Hg₂I₂ precipitates = so this reaction the precipitation reactions
7. Ba(NO₃)₂ + K₂SO₄ -----> BaSO₄ + 2KNO₃
BaSO₄ precipitates = so this reaction the precipitation reactions
<h3>Learn more</h3>
the rate of a chemical reaction
the reducing agent
substance loses electrons in a chemical reaction
Keywords: a double-replacement equation, A single-replacement reaction
You might be interested in
Answer:
a)If concentration of [Sucrose] is changed to 2.5 M than rate will be increased by the factor of 2.5.
b)If concentration of [Sucrose] is changed to 0.5 M than rate will be increased by the factor of 0.5.
c)If concentration of is changed to 0.0001 M than rate will be increased by the factor of 0.01.
d) If concentration when [sucrose] and both are changed to 0.1 M than rate will be increased by the factor of 1.
Explanation:
Sucrose + fructose+ glucose
The rate law of the reaction is given as:
[sucrose]= 1.0 M
..[1]
a)
The rate of the reaction when [Sucrose] is changed to 2.5 M = R'
..[2]
[2] ÷ [1]
If concentration of [Sucrose] is changed to 2.5 M than rate will be increased by the factor of 2.5.
b)
The rate of the reaction when [Sucrose] is changed to 0.5 M = R'
..[2]
[2] ÷ [1]
If concentration of [Sucrose] is changed to 0.5 M than rate will be increased by the factor of 0.5.
c)
The rate of the reaction when is changed to 0.001 M = R'
..[2]
[2] ÷ [1]
If concentration of is changed to 0.0001 M than rate will be increased by the factor of 0.01.
d)
The rate of the reaction when [sucrose] and both are changed to 0.1 M = R'
..[2]
[2] ÷ [1]
If concentration when [sucrose] and both are changed to 0.1 M than rate will be increased by the factor of 1.