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mote1985 [20]
3 years ago
14

How can you describe the location of magnesium (Mg, atomic number 12) periodic table?

Chemistry
2 answers:
olga_2 [115]3 years ago
8 0
The answer is C because it's asking for the location, not the type of element it is like a metal, nonmetal, or metalloid.
icang [17]3 years ago
4 0
A metal group 2 period
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A sample of gas contains 3.0L of nitrogen at 320kPa. What volume would be necessary to decrease the pressure at 110kPa
Phoenix [80]

Answer:

V_{2} = 8.92 L

Explanation:

We have the equation for ideal gas expressed as:

PV=nRT

Being:

P = Pressure

V = Volume

n = molar number

R = Universal gas constant

T = Temperature

From the statement of the problem I infer that we are looking to change the volume and the pressure, maintaining the temperature, so I can calculate the right side of the equation with the data of the initial condition of the gas:

P_{1} V_{1} =nRT

320Kpa*0.003m^{3} =nRT

1000L = 1m^{3}

So

nRT= 0.96

Now, as for the final condition:

P_{2}V_{2}=nRT

P_{2} V_{2} =0.96

clearingV_{2}

V_{2} =\frac{0.96}{P_{2} }

V_{2} =0.00872m_{3}

V_{2} = 8.92 L

6 0
3 years ago
Look at the picture below. Name the isotope.
Aleks [24]

Answer:

carbon-13

Explanation:

6 0
3 years ago
Silicon is used in computers. Give reasons.<br>​
Amanda [17]

Answer:

Silicon is the basic material used to make computer chips, transistors, silicon diodes and other electronic circuits and switching devices because its atomic structure makes the element an ideal semiconductor.

3 0
3 years ago
Read 2 more answers
Be sure to answer all parts. one of the most important industrial sources of ethanol is the reaction of steam with ethene derive
lions [1.4K]

Answer: 2.17x10⁻³ atm

Explanation:

First, we must write the balanced chemical equation for the process:

C₂H₄(g) + H₂O(g) ⇌ C₂H₅OH(g)

The chemical reactions that occur in a closed container can reach a state of <u>chemical equilibrium</u> that is characterized because the concentrations of the reactants and products remain constant over time. The <u>equilibrium constant</u> of a chemical reaction is the value of its reaction quotient in chemical equilibrium.

The equilibrium constant (K) is expressed as <u>the ratio between the molar concentrations (mol/L) of reactants and products.</u> Its value in a chemical reaction depends on the temperature, so it must always be specified.

<u>We will use the the equilibrium constant Kc of the reaction to calculate partial pressure of ethene.</u> The constant Kc for the above reaction is,

Kc = \frac{[C_{2} H_{5}OH]}{[H_{2}O][C_{2} H_{4}]}

According to the law of ideal gases,  

PV = nRT  

where P, V, n and T are the pressure, volume, moles and temperature of the gas in question while R is the gas constant (0.082057 atm L / mol K) .

We can use the ideal gas law to determine the molar concentrations ([x] = n / V) from the gas pressures of ethanol and water, assuming that all gases involved behave as ideal gases. In this way,

PV = nRT → P = (n/V) RT → P = [x] RT → [x] = P / RT

So,  

[C_{2} H_{5}OH] = \frac{200 atm}{0.082057 \frac{atm L}{mol K} x 600 K } = 4.06 \frac{mol}{L}

[H_{2}O] = \frac{400 atm}{0.082057 \frac{atm L}{mol K} x 600 K } = 8.12 \frac{mol}{L}

So, the molar concentration of ethene (C₂H₄) will be,

[C_{2} H_{4}] = \frac{[C_{2} H_{5}OH]}{[H_{2}O] x Kc} = \frac{4.06 \frac{mol}{L} }{8.12 \frac{mol}{L}x9.00 x 10^{3} \frac{L}{mol} } = 5.56 x 10^{-5}\frac{mol}{L}

Then, according to the law of ideal gases,

P_{C_{2} H_{4}} = [C_{2} H_{4}]RT = 5.56 x 10^{-5} \frac{mol}{L}  x 0.082057 \frac{atm L}{mol K} x 600 K = 2.17x10^{-3} atm

So, when the partial pressure of ethanol is 200 atm and the partial pressure of water is 400 atm, the partial pressure of ethene at 600 K is 2.17x10⁻³ atm.

7 0
3 years ago
45. The following data was collected for 3 compounds:
Vika [28.1K]

Answer:

The three compounds are different compounds

Explanation:

The mass of Nitrogen that combines with 1 gram of Oxygen in  Compound A = 1.750 g

The mass of Nitrogen that combines with 1 gram of Oxygen in  Compound B  = 0.8750 g

The mass of Nitrogen that combines with 1 gram of Oxygen in  Compound C  = 0.4375 g

According to the law of multiple proportions, when atoms of two different elements react to form compounds, the masses of one of the elements that combines with a fixed mass of the other element are in small whole number ratios.

The ratio of the masses are;

Mass of Nitrogen in Compound B/(Mass of Nitrogen in Compound C =  0.8750/0.4375 = 2

Mass of Nitrogen in Compound A/(Mass of Nitrogen in Compound C =  1.750/0.4375= 4

Mass of Nitrogen in Compound A/(Mass of Nitrogen in Compound B =  1.750/0.8750= 2

Given that the masses of Nitrogen in the three compounds are in small whole number ratios, the three compounds, Compound A, Compound B, and Compound C are different compounds.

5 0
3 years ago
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