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kirill [66]
3 years ago
9

How much heat is absorbed by a 26g iron skillet when its temperature rises from 13oC to 26oC?

Chemistry
1 answer:
Charra [1.4K]3 years ago
8 0

Answer:- 152.1 J

Solution:-  This type of problems are solved by using the formula:

q=mc\Delta T

where, q is the heat energy, m is the mass, c is specific heat and \Delta T is change in temperature.

mass of iron is given as 26 g. temperature is changing from 13 degree C to 26 degree C.

So, \Delta T = 26 - 13 = 13 degree C

specific heat for iron is 0.450 Joule per gram per degree C.

let's plug in the values in the formula and do calculations for q.

q=26g*\frac{0.450J}{g.^0C}*13^0C

q = 152.1 J

So, 152.1 J of heat is absorbed by the iron skillet.

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How many grams of Cl2 are consumed to produce 12.0 g of KCl?
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The reaction is:

Cl2 + 2 KBr --> 2 KCl + Br2

Moles of KCl is

n = m /M = 12 /74 = 0.16 mol

As, twice the moles of KCl is producing from 1 mol of chlorine

mole of Cl2 = 0.16 /2 = 0.08 mol

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m /70 = 0.08 = 5.6 g

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What is the molarity of a solution that contains 14 moles of solute and 2 liters of solution?
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  7 M

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Why does perchloric acid cause macromolecules to precipitate?
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Directions: Each set of lettered choices below refers to the numbered statements immediately following it. Select the one letter
maksim [4K]

Answer : The only reaction (C) that shows that the same reactant undergoes both oxidation and reduction.

Explanation :

Disproportionation reaction : It is defined as the reaction in which the same reactant undergoes both oxidation and reduction reaction. It is a redox reaction.

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

(A) The given balanced reaction is,

H_2SeO_4(aq)+2Cl^-(aq)+2H^+(aq)\rightarrow H_2SeO_3(aq)+Cl_2(g)+H_2O(l)

This reaction is a redox reaction but not disproportionation reaction because in this reaction there are two reactants in which chlorine shows oxidation and selenium shows reduction.

(B) The given balanced reaction is,

S_8(s)+8O_2(g)\rightarrow 8SO_2(g)

This reaction is a redox reaction but not disproportionation reaction because in this reaction there are two reactants in which sulfur shows oxidation and oxygen shows reduction.

(C) The given balanced reaction is,

3Br_2(aq)+6OH^-(aq)\rightarrow 5Br^-(aq)+BrO_3^-(aq)+3H_2O(l)

This reaction is a disproportionation reaction because in this reaction only one reactant bromine that shows both oxidation and reduction reaction.

(D) The given balanced reaction is,

Ca^{2+}(aq)+SO_4^{2-}(aq)\rightarrow CaSO_4(s)

This reaction is a combination reaction in which the two reactant react to give a single product. There is no changes in the oxidation state of calcium and sulfate.

(E) The given balanced reaction is,

PtCl_4(s)+2Cl^-(aq)\rightarrow PtCl_6^{2-}(aq)

This reaction is a combination reaction in which the two reactant react to give a single product. There is no changes in the oxidation state of platinum and chlorine.

Hence, the only reaction (C) that shows that the same reactant undergoes both oxidation and reduction.

6 0
3 years ago
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