Air is a solution of gases, what is the solvent in air?

ddd [48]

Its the very last option i believe

5 0

3 years ago

A motor uses the attracting and repelling forces of magnets to create rotational motion. What type of energy results from this p

zavuch27 [327]

b) Mechanical

:D Hope it helps!

7 0

3 years ago

Read 2 more answers

The balanced equation for the reaction between iron sulfied and water is best represented by?

nika2105 [10]

FeS + H₂O → FeO + H₂S

Explanation:

Iron Sulfide = FeS

Water = H₂O

FeS + H₂O → FeO + H₂S

To balance this equation, we can use a mathematical method. This involves solving simple algebraic equations

aFeS + bH₂O → cFeO + dH₂S

a,b,c and d are the coefficients needed to balance up the equation:

Conserving Fe: a = c

S: a = d

H: 2b = 2d

O: b = c

let a = 1, c= 1, b = 1 d = 1

The balanced equation is: FeS + H₂O → FeO + H₂S

learn more:

Balanced equation brainly.com/question/2612756

#learnwithBrainly

4 0

3 years ago

How hydrogen chloride gas is prepared on labrotary by conc sulpheric acid<br>

Citrus2011 [14]

Answer:

It is prepared small amounts of hydrogen cloride for uses in the lab.

It can be "generated in an HCl generator by dehydrating hydrochloric acid with either sulfuric acid or anhydrous calcium chloride."

4 0

3 years ago

The equilibrium constant for the reaction AgBr(s) Picture Ag+(aq) + Br− (aq) is the solubility product constant, Ksp = 7.7 × 10−

barxatty [35]

Answer:

The reaction will be non spontaneous at these concentrations.

Explanation:

$AgBr(s)\rightarrow Ag^+(aq) + Br^- (aq)$

Expression for an equilibrium constant $K_c$ :

$K_c=\frac{[Ag^+][Br^-]}{[AgCl]}=\frac{[Ag^+][Br^-]}{1}=[Ag^+][Br^-]$

Solubility product of the reaction:

$K_{sp}=[Ag^+][Br^-]=K_c=7.7\times 10^{-13}$

Reaction between Gibb's free energy and equilibrium constant if given as:

$\Delta G^o=-2.303\times R\times T\times \log K_c$

$\Delta G^o=-2.303\times R\times T\times \log K_{sp}$

$\Delta G^o=-2.303\times 8.314 J/K mol\times 298 K\times \log[7.7\times 10^{-13}]$

$\Delta G^o=69,117.84 J/mol=69.117 kJ/mol$

Gibb's free energy when concentration $[Ag^+] = 1.0\times 10^{-2} M$ and $[Br^-] = 1.0\times 10^{-3} M$

Reaction quotient of an equilibrium = Q

$Q=[Ag^+][Br^-]=1.0\times 10^{-2} M\times 1.0\times 10^{-3} M=1.0\times 10^{-5}$

$\Delta G=\Delta G^o+(2.303\times R\times T\times \log Q)$

$\Delta G=69.117 kJ/mol+(2.303\times 8.314 Joule/mol K\times 298 K\times \log[1.0\times 10^{-5}])$

$\Delta G=40.588 kJ/mol$

For reaction to spontaneous reaction: $\Delta G$ .
For reaction to non spontaneous reaction: $\Delta G>0$ .

Since ,the value of Gibbs free energy is greater than zero which means reaction will be non spontaneous at these concentrations

5 0

3 years ago