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4 years ago

Which choice is characterized by being malleable? A. metaloids B. metals C. noble gases D. nonmetals

Chemistry

2 answers:

Ainat [17]4 years ago

4 0

The correct answer is metals

amid [387]4 years ago

4 0

Answer: option B. metals.

Justification:

1) Elements can be classified into three main categories: metals, nonmetals, and metaloids.

The metals constitute the most of the elements, which you can see in a periodic table.

2) Most metals are ductiles and malleables, which means that they can be formed into thin sheets and wires.

3) The nonmetals are either gases or brittle solids, ergo they are not malleables.

4) Metalloids have some metallic properties, son nonmetallic properties, and some intermediate properties. They are not malleable nor ductile. There are only 8 metalloids: boron, silicon, germanium, arsenic, antimony, tellurium, polonium and astatine. They are brittle.

The malleabillity is a typical property of the metals.

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If a neutral atom becomes negatively charged, it has undergone _________.

ycow [4]

If a neutral atom becomes negatively charged, it has undergone reduction.

Reduction is the process through which a neutral atom gain an electron (thus reducing its oxidation number) and turns into a negative ion (also known as : anion)

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3 years ago

Phosgene, COCl2, gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide w

jek_recluse [69]

The question is incomplete, here is the complete question:

Phosgene, $COCl_2$ , gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:

$CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

The value of $K_c$ for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which $p_{CO}=p_{Cl_2}=0.265atm$ and $p_{COCl_2}=0.000atm$ ?

Answer: The equilibrium partial pressure of CO, $Cl_2\text{ and }COCl_2$ is 0.257 atm, 0.257 atm and 0.008 atm respectively.

Explanation:

The relation of $K_c\text{ and }K_p$ is given by:

$K_p=K_c(RT)^{\Delta n_g}$

$K_p$ = Equilibrium constant in terms of partial pressure

$K_c$ = Equilibrium constant in terms of concentration = 5.79

$\Delta n_g$ = Difference between gaseous moles on product side and reactant side = $n_{g,p}-n_{g,r}=1-2=-1$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

T = Temperature = 570 K

Putting values in above equation, we get:

$K_p=5.79\times (0.0821\times 570)^{-1}\\\\K_p=0.124$

We are given:

Initial partial pressure of CO = 0.265 atm

Initial partial pressure of chlorine gas = 0.265 atm

Initial partial pressure of phosgene = 0.00 atm

The given chemical equation follows:

$CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)$

Initial: 0.265 0.265

At eqllm: 0.265-x 0.265-x x

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{COCl_2}}{p_{CO}\times p_{Cl_2}}$

Putting values in above equation, we get:

$0.124=\frac{x}{(0.265-x)\times (0.265-x)}\\\\x=0.0082,8.59$

Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure

So, the equilibrium partial pressure of CO = $(0.265-x)=(0.265-0.008)=0.257atm$

The equilibrium partial pressure of $Cl_2=(0.265-x)=(0.265-0.008)=0.257atm$

The equilibrium partial pressure of $COCl_2=x=0.008atm$

Hence, the equilibrium partial pressure of CO, $Cl_2\text{ and }COCl_2$ is 0.257 atm, 0.257 atm and 0.008 atm respectively.

6 0

3 years ago

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IRISSAK [1]

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Andru [333]

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3 years ago

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