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3 years ago

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Calculate the specific heat capacity of a piece of ice if 1.30 kg of the wood absorbs 6.75×104 joules of heat, and its temperatu

re changes from 32 ºC to 57 ºC.

2 answers:

spayn [35]3 years ago

8 0

Answer:

1.8 J/ g ∘ C

Explanation:

A substance's specific heat tells you how much heat much either be added or removed from 1 g of that substance in order to cause a 1 ∘ C change in temperature.

The equation that establishes a relationship between specific heat, heat added or removed.

Lunna [17]3 years ago

5 0

Answer:

2076.9 J/kg°C

Explanation:

The equation needed here is:

$q=mC(T_f-T_i)$ , where q is the energy in Joules, m is the mass in kg, C is the heat capacity, T_f is the final temperature, and T_i is the initial temperature.

Here, we have q = 6.75* $10^4$ J, m = 1.30kg, T_f = 57, and T_i = 32. So:

$6.75*10^4=1.30*C*(57-32)$

Solving for C, we get:

C = 2076.9 J/kg°C

Hope this helps!

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Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. None of the above pairs will

Alla [95]

Answer:

Only $Fe^{3+}+Mg$ gives spontaneous reaction.

Explanation:

A redox reaction will be spontaneous if standard reduction potential ( $E^{0}$ ) of the reaction is positive. Because it leads to negative standard gibbs free energy change ( $\Delta G^{0}$ ), which is a thermodynamic condition for spontaneity of a reaction.

$E^{0}=E^{0}(reduction)-E^{0}(oxidation)$

Where $E^{0}(reduction)$ and $E^{0}(oxidation)$ represents standard reduction potential of reduction half cell and standard reduction potential of oxidation half cell.

(1) Oxidation: $Mg-2e^{-}\rightarrow Mg^{2+}$ ; $E_{Mg^{2+}\mid Mg}^{0}=-2.38V$

Reduction: $Fe^{3+}+3e^{-}\rightarrow Fe$ ; $E_{Fe^{3+}\mid Fe}^{0}=-0.04V$

So, $E^{0}=E_{Fe^{3+}\mid Fe}^{0}-E_{Mg^{2+}\mid Mg}^{0}=(-0.04+2.38)V=2.34V$

Hence this pair will give spontaneous reaction.

(2) Similarly as above, $E^{0}=E_{Pb^{2+}\mid Pb}^{0}-E_{Au^{+}\mid Au}^{0}=(-0.13-1.69)V=-1.82 V$

Hence this pair will give non-spontaneous reaction.

(3) Similarly as above, $E^{0}=E_{Ag^{+}\mid Ag}^{0}-E_{Br_{2}\mid Br^{-}}^{0}=(0.80-1.07)V=-0.27 V$

Hence this pair will give non-spontaneous reaction.

(4) Similarly as above, $E^{0}=E_{Li^{+}\mid Li}^{0}-E_{Cr^{3+}\mid Cr}^{0}=(-3.04+0.74)V=-2.30 V$

Hence this pair will give non-spontaneous reaction.

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Answer:

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2 years ago

Automobile bodies contain significant amounts of iron. The iron is protected by the addition of zinc. This is called galvanizati

Oksana_A [137]

<u>Answer:</u> The balanced chemical equation is written below.

<u>Explanation:</u>

Galvanization is defined as the process in which a protective layer of zinc is applied to iron or steel to prevent the metal from rusting.

Zinc prevents the oxidation of iron and acts as a reducing agent in the process.

The half reaction for the process follows:

<u>Oxidation half reaction:</u> $Zn\rightarrow Zn^{2+}+2e^-$

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Net chemical equation: $Zn+Fe^{2+}\rightarrow Zn^{2+}+Fe$

Hence, the balanced chemical equation is written above.

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3 years ago