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Harrizon [31]
3 years ago
9

Copper(i) ions in aqueous solution react with nh3(aq) according to

Chemistry
1 answer:
Vlada [557]3 years ago
6 0
The complete question is; copper (i) ions in aqueous solutions react with NH3(aq) according to;
 Cu +2NH3 = Cu(NH3)2    Kt= 6.3 × 10^10
Calculate K
Cu + 2NH3 = Cu(NH3)2
kf = 6.3 ×10^10
The ksp for CuBr = Cu + Br = 6.3 × 10^-9
For the reaction; CuBr +2NH3 = Cu(NH3)2 + Br to calculate K?
K = (6.3 × 10^10)(6.3×10^-9) 
Thus K is 396.9 
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This is a measure of mass per unit volume.
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Answer:

Density

Explanation:

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What action leads to crystal formation in minerals?
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Write a net ionic equation for the reaction that occurs when aqueous solutions of nitric acid and sodium hydroxide are combined.
Veronika [31]

Answer:

H^+(aq) +  OH^-(aq) -------> H2O(l)

Explanation:

We must first write the molecular reaction equation as follows;

HNO3(aq) + NaOH(aq) ------>NaNO3(aq) + H2O(l)

The complete ionic equation is;

H^+(aq) + NO3^-(aq) + Na^+(aq) + OH^-(aq) -------> Na^+(aq) + NO3^-(aq) + H2O(l)

The net ionic equation therefore is;

H^+(aq) +  OH^-(aq) -------> H2O(l)

5 0
3 years ago
Example of market structures of monopoly
IgorC [24]

Answer: A monopoly is the absence of competition in the market.

Explanation:

In such circumstances, the market creates a monopoly of one producer who takes huge capital and dictates prices. An example of a monopoly on the market is the existence of only one company that makes up the entire economic branch. In such circumstances, the monopolist can increase the product's price without losing the entire sale, i.e., operating successfully. In that situation, the monopolist remains the only one on the market, and the competition has no access to the market.

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3 years ago
The standard enthalpy of reaction for the dissolution of silica in aqueous HF is 4.6 kJ mol–1 . What is the standard enthalpy of
Stels [109]

Answer:

B) ) –1615.1 kJ mol^–1

Explanation:

since

SiO2(s) + 4 HF(aq) → SiF4(g) + 2 H2O(l) ∆Hºrxn = 4.6 kJ mol–1

the enhalpy of reaction will be

∆Hºrxn = ∑νp*∆Hºfp - ∑νr*∆Hºfr

where ∆Hºrxn= enthalpy of reaction , ∆Hºfp= standard enthalpy of formation of products , ∆Hºfr = standard enthalpy of formation of reactants , νp=stoichiometric coffficient of products, νr=stoichiometric coffficient of reactants

therefore

∆Hºrxn = ∑νp*∆Hºfp - ∑νr*∆Hºfr

4.6 kJ/mol = [1*∆HºfX + 2*(–285.8 kJ/mol)] - [1*(–910.9kJ/mol) + 4*(–320.1 kJ/mol)]

4.6 kJ/mol =∆HºfX -571.6 kJ/mol + 2191.3 kJ/mol

∆HºfX = 4.6 kJ/mol + 571.6 kJ/mol - 2191.3 kJ/mol = -1615.1 kJ/mol

therefore ∆HºfX (unknown standard enthalpy of formation = standard enthalpy of formation of SiF4(g) ) = -1615.1 kJ/mol

8 0
3 years ago
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