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3 years ago

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Which type of substance can conduct electricity in the liquid phase but not in the solid phase and why?

2 answers:

Citrus2011 [14]3 years ago

3 0

1) ionic compound

there should be motive ions or free movable electrons to conduct electricity. The ionic compounds in the solid state, has no motive ions or free electrons as the ions are tightly attracted to each other. But in liquid state, the ions separate and move freely.

stepladder [879]3 years ago

3 0

Answer:ionic compound

Explanation:

In an ionic solid, all the ions are tightly held by electrostatic attraction with the neighbouring oppositely charged ion hence they are immobile. Electricity conduction by ionic substances depends on the mobility of ions. When dissolved in water, these ions are now pulled apart from each other and migrate freely. The same occurs when the crystal lattice collapses and the solid melts. Hence only the fused substance or the solution of the substance can conduct electricity.

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Consider the reaction. PCl5(g)↽−−⇀PCl3(g)+Cl2(g) K=0.042 The concentrations of the products at equilibrium are [PCl3]=0.18 M and

tatyana61 [14]

<u>Answer:</u> The equilibrium concentration of $PCl_5$ is 1.285 M.

<u>Explanation:</u>

The chemical equation for the decomposition of phosphorus pentachloride follows:

$PCl_5(g)\rightleftharpoons PCl_3(g)+Cl_2(g)$

The expression for equilibrium constant is given as:

$K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}$

We are given:

$K_c=0.042$

$[PCl_3]=0.18M$

$[Cl_2]=0.30M$

The concentration of solid substances are taken to be 1. Thus, they do not appear in the equilibrium constant expression.

Putting values in above equation, we get:

$0.042=\frac{0.18\times 0.30}{[PCl_5]}$

$[PCl_5]=1.285$

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3 years ago

A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ros

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<h3>Answer:</h3>

A) -1.24 × 10^3 kJ/Mol

<h3>Explanation:</h3>

we are given;

Mass of ethanol, m = 35.6 g

Temperature change, Δt(35.0 to 76.0°C) = 41 °C

Specific heat capacity of the calorimeter, c = 23.3 kJ/°C

Molar mass of ethanol = 46.07 g/mol

We are required to the heat change of the reaction.

We need to note that the reaction is an exothermic reaction since there is an increase in temperature which means heat was lost to the surroundings.

Therefore; we are going to use the following steps;

<h3>Step 1 : Moles of ethanol </h3>

We know, Moles = Mass ÷ molar mass

Thus, moles of ethanol = 35.6 g ÷ 46.07 g/mol

= 0.773 moles

<h3>Step 2: Enthalpy change or heat change for the reaction.</h3>

Heat change = -mcΔt

but we are given s[pecific heat capacity in Kj/°C and we require heat change in kJ/mol

Therefore;

Heat change = -(cΔt) ÷ n ( n is the number of moles)

= -( 23.3 kJ/°C × 41°C) ÷0.773 mol

= - 1.24 × 10^3 kJ/Mol

Therefore, values of ΔH of the reaction is -1.24 × 10^3 kJ/Mol

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3 years ago