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3 years ago

Is this sentence true or false ? hydrogen is considered to be a metal

Chemistry

2 answers:

blsea [12.9K]3 years ago

8 0

It is considered to be because of its similarities in electrons but ultimately it is not.

victus00 [196]3 years ago

4 0

It is false, hope this helps!

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The molar heat of vaporization for methane, CH4, is 8. 53 kJ/mol. How much energy is absorbed when 54. 8 g of methane vaporizes

alexandr402 [8]

Molar heat of vaporization is defined as the heat absorbed by one mole of substance to convert from liquid to gas.

<h3>How do you calculate the heat of vaporization?</h3>

The formula used to calculate the heat of vaporization is:

$\rm Q &= n \times \Delta H$

Where,

Q = Amount of Heat

n = number of moles of a substance

$\Delta H =$ molar enthalpy of fusion

Now, to calculate the moles of methane:

$\rm Moles &= \dfrac{Mass \;of\; methane }{Molar\; Mass\; of \; Methane} &= \dfrac{54.8\;g}{16\;g/mol}$

Moles = 3.425 mol

Now, 1 mol of methane absorbs = 8.53 KJ

3.425 mol of methane absorbs = $3.424 \times 8.53 &= 29.1 KJ$

Thus, the energy is absorbed till the methane vaporizes at its boiling point is 29.1 KJ.

Learn more about vaporization here:

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2 years ago

Balance the following equations:

neonofarm [45]

Hope this helps! If you dont understand balancing equations in general, say so in the comments, I’m happy to help

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3 years ago

Help me please I really do need help pls text me if u wanna help me more

8090 [49]

Respiration . I’m pretty sure

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3 years ago

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makvit [3.9K]

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3 years ago

What volume of nitrogen dioxide is formed at 735 torr and 28.2 °C by reacting 3.56 cm3 of copper (d = 8.95 g/cm3) with 200 mL of

weqwewe [10]

Answer:

25.76 L

Explanation:

Given, Volume of Copper = 3.56 cm³

Density = 8.95 g/cm³

Considering the expression for density as:

$Density=\frac {Mass}{Volume}$

So,

So, Mass= Density * Volume = 8.95 g/cm³ * 3.56 cm³ = 31.862 g

Mass of copper = 31.862 g

Molar mass of copper = 63.546 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{31.862\ g}{63.546\ g/mol}$

Moles of copper = 0.5014 moles

Given, Volume of nitric acid solution = 200 mL = 200 cm³

Density = 1.42 g/cm³

Considering the expression for density as:

$Density=\frac {Mass}{Volume}$

So,

So, Mass= Density * Volume = 1.42 g/cm³ * 200 cm³ = 284 g

Also, Nitric acid is 68.0 % by mass. So,

Mass of nitric acid = $\frac {68}{100}\times 284\ g$ = 193.12 g

Molar mass of nitric acid = 63.01 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{193.12\ g}{63.01\ g/mol}$

Moles of nitric acid = 3.0649 moles

According to the reaction,

$Cu_{(s)}+4HNO_3_{(aq)}\rightarrow Cu(NO_3)_2_{(aq)} + 2NO_2_{(g)} + 2H_2O_{(l)}$

1 mole of copper react with 4 moles of nitric acid

Thus,

0.5014 moles of copper react with 4*0.5014 moles of nitric acid

Moles of nitric acid required = 2.0056 moles

Available moles of nitric acid = 3.0649 moles

Limiting reagent is the one which is present in small amount. Thus, nitric acid is present in large amount, copper is the limiting reagent.

The formation of the product is governed by the limiting reagent. So,

1 mole of copper on reaction forms 2 moles of nitrogen dioxide

So,

0.5014 mole of copper on reaction forms 2*0.5014 moles of nitrogen dioxide

Moles of nitrogen dioxide = 1.0028 moles

Given:

Pressure = 735 torr

The conversion of P(torr) to P(atm) is shown below:

$P(torr)=\frac {1}{760}\times P(atm)$

So,

Pressure = 735 / 760 atm = 0.9632 atm

Temperature = 28.2 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T₁ = (28.2 + 273.15) K = 301.35 K

Using ideal gas equation as:

PV=nRT

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L.atm/K.mol

Applying the equation as:

0.9632 atm × V = 1.0028 mol × 0.0821 L.atm/K.mol × 301.35 K

⇒V = 25.76 L

4 0

3 years ago