All categories

3 years ago

Can anyone do balance equation?

Chemistry

1 answer:

miss Akunina [59]3 years ago

3 0

47)1-6 and 5&6-8 hope this helps!

You might be interested in

The distance measured between five successive crests of a wave motion executed by a photon of an electromagnetic radiation is 2.

Jet001 [13]

Answer:

6.25 ×10^10 Hz

Explanation:

If the distance between five successive crests is 2.4 cm, then the distance between each crest is 2.4/5 = 0.48 cm or 0.0048 m or 4.8 ×10^-3 m

Since the velocity of a wave is given by;

v= λf

Where;

λ= wavelength of the wave

f= frequency of the wave

But λ= distance between successive crests = 4.8 ×10^-3 m

v= 3×10^8 ms-1 (speed of electromagnetic waves in vacuum)

f= v/λ

f= 3×10^8 ms-1/4.8 ×10^-3 m

f= 0.625 ×10^11 Hz

f= 6.25 ×10^10 Hz

6 0

3 years ago

If the s and p sublevels of the highest main energy level of an atom are filled, how many

Anuta_ua [19.1K]

Answer:

Explanation:

8 0

3 years ago

Why are redox reactions used in batteries?

Lelechka [254]

Answer:

The attraction between charged ions releases energy. The movement of electrons creates an electric current. Dont put down the same exact awser that i did.

Explanation:

6 0

4 years ago

Read 2 more answers

Determine the concentration of nh3(aq) that is required to dissolve 743 mg of agcl(s) in 100.0 ml of solution. the ksp of agcl i

AnnyKZ [126]

Answer:

1.1 M

Explanation:

The dissociation of $AgCl_{(s)}$ is as follows:

$AgCl \leftrightharpoons Ag^+_{(aq)}+Cl^-_{(aq)}$

Given Value for $K_{sp} = 1.77*10^{-10}$

The equation for the reaction for the formation of complex ion $Ag(NH_3)^+_2$ is :

$Ag^+_{(aq)} + 2NH_3_{(aq)} \rightleftharpoons Ag(NH_3)_2^+_{(aq)}$

The value of $K_f = 1.6*10^7$

If we combine both equation and find the overall equilibrium constant will be:

$AgCl \leftrightharpoons Ag^+_{(aq)}+Cl^-_{(aq)}$

$Ag^+_{(aq)} + 2NH_3_{(aq)} \rightleftharpoons Ag(NH_3)_2^+_{(aq)}$

$AgCl_{(s)}+2NH_3_{(aq)} \rightleftharpoons Ag(NH_3)_2^+_{(aq)} + Cl^-_{(aq)}$

$K = (1.77*10^{-10})(1.6*10^7)$

$K = 0.00283$

If $[NH_3]$ = x M

The solubility of $AgCl_{(s)}$ in the $NH_3$ solution will be:

$x = 743*10^{-3}g * \frac{mol AgCl}{143.32g}*\frac{1}{0.1000L}$

$x = 0.0518 M$

Constructing an ICE Table; we have :

$AgCl_{(s)} + 2 NH_3{(aq)} \rightleftharpoons Ag(NH_3)_2^+_{(aq)} + Cl^-_{(aq)}$

Initial (M) x 0 0

Change (M) -2 (0.0518) + 0.0518 + 0.0518

Equilibrium (M) x - 0.1156 0.0518 0.0518

Equilibrium constant;

(K) = $\frac{[Ag(NH_3)_2^+][Cl^-]}{[NH_3]^2}$

$0.00283 = \frac{(0.0518)^2}{(x-0.1156)^2}$

$0.00283 = (\frac{0.0518}{x-0.1156})^2$

$x = 0.1156 + \sqrt{\frac{0.0518^2}{0.00283} }$

x = [NH₃] = 1.089 M

[NH₃] ≅ 1.1 M

8 0

3 years ago

A kid falling out of a tree, what type of energy conversions are occurring

Valentin [98]

Potential to kinetic

6 0

3 years ago