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astra-53 [7]
1 year ago
7

question 7 a data analyst is creating a visualization in tableau public. they want to keep it private from other users until it

is complete. which icon should they click? 1 point close eye source private
Chemistry
1 answer:
Leona [35]1 year ago
7 0

To keep the data private from the public, the user should use the c)eye icon.

The Eye icon helps users to keep their visualizations private from other users. When clicked, it makes the visualization inaccessible to other users.

This helps ensure that the visualization is only visible to the user who created it and not to anyone else. Additionally, the Eye icon also helps prevent accidental deletion or modification of the visualization.

When the visualization is private, it is not visible to other users until the Eye icon is clicked again to make the visualization public. This makes it easier for the user to control who can access their visualization and helps protect their data.

Therefore, the correct option is c and the icon is the eye.

To know more about data science and interpretation, click below:

brainly.com/question/13104055

#SPJ4

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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

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