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Serhud [2]
3 years ago
13

What is true about a block of ice at -10 degrees celsius as you continue to apply heat...

Chemistry
1 answer:
Y_Kistochka [10]3 years ago
4 0

A. Its temperature will rise continuously until it completely melts

I don't believe that any of the other answers are correct because the ice cannot stay at a certain temperature if it is melting.

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Given the balanced equation representing a reaction:
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Complete the sentensent.Use the present simple or the present continuous.
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Determine the free energy(ΔG) from the standard cell potential (Ecell0 ) for the reaction:2ClO2-(aq)+Cl2(g)→2ClO2(g)+ 2Cl-(aq)wh
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<u>Answer:</u> The \Delta G^o for the given reaction is -7.84\times 10^4J

<u>Explanation:</u>

For the given chemical reaction:

2ClO_2^-(aq.)+Cl_2(g)\rightarrow 2ClO_2(g)+2Cl^-(aq.)

Half reactions for the given cell follows:

<u>Oxidation half reaction:</u> ClO_2^-\rightarrow ClO_2+e^-;E^o_{ClO_2^-/ClO_2}=0.954V  ( × 2)

<u>Reduction half reaction:</u> Cl_2+2e^-\rightarrow 2Cl(g);E^o_{Cl_2/2Cl^-}=1.36V

Oxidation reaction occurs at anode and reduction reaction occurs at cathode.

To calculate the E^o_{cell} of the reaction, we use the equation:

E^o_{cell}=E^o_{cathode}-E^o_{anode}

Putting values in above equation, we get:

E^o_{cell}=1.36-(0.954)=0.406V

To calculate standard Gibbs free energy, we use the equation:

\Delta G^o=-nFE^o_{cell}

Where,

n = number of electrons transferred = 2

F = Faradays constant = 96500 C

E^o_{cell} = standard cell potential = 0.406 V

Putting values in above equation, we get:

\Delta G^o=-2\times 96500\times 0.406=-78358J=-7.84\times 10^4J

Hence, the \Delta G^o for the given reaction is -7.84\times 10^4J

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3 years ago
Hypothesis and Data Collection Part A The image shows three different liquids: water, water with salt, and vinegar. The pH of ea
Norma-Jean [14]

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The water would be neutral, (usually 7). The salt water would be the same (7) and the vinegar would be very acidic. (probably 2).

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7 0
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