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worty [1.4K]
3 years ago
11

If a 95.0 gram sample of metal at 100.0 oC is placed in 50.0 g of water with an initial temperature of 22.5oC and the final temp

erature of the system is 48.5oC, what is the specific heat of the metal? Group of answer choices
Chemistry
1 answer:
kaheart [24]3 years ago
8 0

Answer : The specific heat of the metal is, 1.11J/g^oC

Explanation

In this problem we assumed that heat given by the hot body is equal to the heat taken by the cold body.

q_1=-q_2

m_1\times c_1\times (T_f-T_1)=-m_2\times c_2\times (T_f-T_2)

where,

c_1 = specific heat of metal = ?

c_2 = specific heat of water = 4.18J/g^oC

m_1 = mass of metal = 95.0g

m_2 = mass of water  = 50.0 g

T_f = final temperature of mixture = 48.5^oC

T_1 = initial temperature of metal = 100.0.0^oC

T_2 = initial temperature of water = 22.5^oC

Now put all the given values in the above formula, we get

(95.0g)\times c_1\times (48.5-100.0)^oC=-[(50.0g)\times 4.18J/g^oC\times (48.5-22.5)^oC]

c_1=1.11J/g^oC

Therefore, the specific heat of the metal is, 1.11J/g^oC

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Answer:

The magnesium will burn until consumed entirely. There is much more oxygen available in the atmosphere than needed to consume the magnesium. Thus the magnesium is the limiting reactant because it determines the amount of product formed.

Explanation:

Mg produces less amount of MgO than O2; therefore Mg is the limiting reagent. O2 produces more amount of MgO than Mg; therefore O2 is the excess reagent.

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3 years ago
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

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Answer:

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The process of cytokinesis is different for animal cell and plant cell.

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Hence, from the given information of the question,

The correct answer is animal cell.

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Procedures that are likely a chemical change are:

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4. implementing

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