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3 years ago

Which metalloids would behave more like metals? Which metalloids would behave more like nonmetals?.

Chemistry

2 answers:

joja [24]3 years ago

5 0

The metalloid that tends to act more like metals is boron.

The metalloids that tend to act more like nonmetals are arsenic, antimony, and tellurium.

Metals are the elements that have the ability to lose electrons, while nonmetals are the elements with the ability to gain electrons.

<h3>Metalloids, Metals, and Nonmetals</h3>

The metalloids are the elements with the ability to act as both metals and nonmetal. The metalloids have wide application, with its characteristic in between metals and nonmetals.

The metalloids with less than 4 electrons in the valence shell tends to act like metals, while metalloids with more than 4 valence electrons tends to act more like nonmetals.

The metalloid that tends to act more like metals is boron.

The metalloids that tend to act more like nonmetals are arsenic, antimony, and tellurium.

Learn more about metalloids, here:

brainly.com/question/17482288

weeeeeb [17]3 years ago

3 0

Answer: A. metalloids in group 16 and B. metalloids in group 13

Explanation: took the test and got it right

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In a first-order decomposition reaction, 50.0% of a compound decomposes in 10.5 min.

mihalych1998 [28]

In this reaction 50% of the compound decompose in 10.5 min thus, it is half life of the reaction and denoted by symbol $t_{1/2}$ .

(a) For first order reaction, rate constant and half life time are related to each other as follows:

$k=\frac{0.6932}{t_{1/2}}=\frac{0.6932}{10.5 min}=0.066 min^{-1}$

Thus, rate constant of the reaction is $0.066 min^{-1}$ .

(b) Rate equation for first order reaction is as follows:

$k=\frac{2.303}{t_{1/2}}log\frac{[A_{0}]}{[A_{t}]}$

now, 75% of the compound is decomposed, if initial concentration $[A_{0} ]$ is 100 then concentration at time t $[A_{t} ]$ will be 100-75=25.

Putting the values,

$0.066 min^{-1}=\frac{2.303}{t}log\frac{100}{25}=\frac{2.303}{t}(0.6020)$

On rearranging,

$t=\frac{2.303\times 0.6020}{0.066 min^{-1}}=21 min$

Thus, time required for 75% decomposition is 21 min.

8 0

3 years ago

Calculate the total pressure in a 10.0 liter flask at 27°C of a sample of gas that contains 6.0 grams of hydrogen, 15.2 grams of

motikmotik

Answer:

The total pressure is 27.8 atm

Explanation:

From the ideal gas equation,

PV = nRT

P (total pressure) = nRT/V

n (total moles of gases) = (6/1 moles of hydrogen) + (15.2/14 moles of nitrogen) + (16.8/4 moles of helium) = 6+1.1+4.2 = 11.3 moles

R = 0.082057L.atm/gmol.K, T = 27°C = 27+273K = 300K, V = 10L

P = 11.3×0.082057×300/10 = 27.8 atm

7 0

3 years ago

What is true if a liquid and a gas are in equilibrium?

MAXImum [283]

Answer:

A - Liquid molecules forming a gas and gas molecules forming a

liquid are equal in number.

Explanation:

A P E X

6 0

3 years ago

Question 21

Mumz [18]

There are 2 moles of O stones present in 88 grams of CO2. Why? Well, we can find the amount of moles present in 88 grams of CO2 by dividing the mass by the molar mass. The mass of CO2 comes out to be 88 grams. The molar mass of CO2 comes out to be 44 grams. Because 88 is the mass of CO2 and 44 is the molar mass of CO2, we can divide 88 by 44 to identify that there are 2.0 moles of O atoms present in 88 grams of CO2.

Your final answer: There are 2.0 moles of O atoms present in 88 grams of CO2. Your final answer to this question is D, or 2.0 moles. If you need to better understand, let me know and I will gladly assist you.

5 0

2 years ago

What volume does 0.482 mol of gas occupy at a pressure of 719 mmHg at 56 ∘C?

kozerog [31]

Answer:

The volume is 13, 69 L

Explanation:

We use the formula PV=nRT. We convert the temperature in Celsius into Kelvin and the pressure in mmHg into atm.

0°C= 273K---> 56°C= 56 + 273= 329K

760 mmHg----1 atm

719 mmHg----x= (719 mmHgx 1 atm)/760 mmHg= 0,95 atm

PV=nRT ---> V= (nRT)/P

V=( 0,482 molx 0,082 l atm/K mol x 329K)/0,95 atm

7 0

3 years ago