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2 years ago

A solid is 5 cm tall 3 cm wide and 2 cm thick it has a mass of 129 g what is the density

2 answers:

7 0

First you would multiply 5,3, and 2 to get a volume of 30. Density is mass over volume so you would then divide 129 by 30. You would get 4.3. The answer would be 4.3 g/cm^3

dlinn [17]2 years ago

4 0

Answer: The density of solid is $4.3g/cm^3$

Explanation:

To calculate the volume of cuboid, we use the equation:

$V=lbh$

where,

V = volume of cuboid

l = length of cuboid = 5 cm

b = breadth of cuboid = 3 cm

h = height of cuboid = 2 cm

Putting values in above equation, we get:

$V=5\times 3\times 2=30cm^3$

To calculate density of a substance, we use the equation:

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

Putting values in above equation, we get:

$\text{Density of solid}=\frac{129g}{30cm^3}\\\\\text{Density of solid}=4.3g/cm^3$

Hence, the density of solid is $4.3g/cm^3$

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Dimethylhydrazine is a carbon-hydrogen-nitrogen compound used in rocket fuels. When burned in an excess of oxygen, a 0.312 gg sa

Stolb23 [73]

Answer:

CH₄N

Explanation:

Given that;

mass of the sample = 0.312 g

mass of CO2 = 0.458 g

mass of H2O = 0.374 g

nitrogen content of a 0.486 gg sample is converted to 0.226 gg N2N2.

Let start with calculating the respective numbers of moles of Carbon Hydrogen and Nitrogen from the given data.

numbers of moles of Carbon from CO2 = $\frac{mass of CO_2}{molarmass}*\frac{1 mole of C}{1 mole of CO_2}$

= $\frac{0.458}{44}*\frac{1mole of C}{1 mole of CO_2}$

= 0.0104 mole

numbers of moles of hydrogen from H2O = $\frac{mass of H_2O}{molarmass}*\frac{2 mole of H}{1 mole of H_2O}$

= $\frac{0.374}{18.02}*\frac{2 mole of H}{1 mole of H_2O}$

= 0.02077 × 2

= 0.0415 mole

The nitrogen content of a 0.486 g sample is converted to 0.226 g N2

Now, in 1 g of the sample; The nitrogen content = $\frac{0.226}{0.486}*1$

in 0.312 g of the sample, the nitrogen content will be; $\frac{0.226}{0.486}*0.312$

= 0.1450 g of N2

number of moles of N2 = $\frac{mass}{molar mass}* \frac{2 mole}{1 mole}$

= $\frac{0.1450}{28.0134} *\frac{2 mole}{1 mole}$

= 0.0103 mole

Finally to determine the empirical formula of Carbon Hydrogen and Nitrogen; we have:

Carbon Hydrogen Nitrogen

number of moles 0.0104 0.0415 0.0103

divided by the

smallest number $\frac{0.0104}{0.0103}$ $\frac{0.0415}{0.0103}$ $\frac{0.0103}{0.0103}$

of moles

1 : 4 : 1

∴ The empirical formula = CH₄N

8 0

2 years ago

Choose the statements about benzene that are correct.

FromTheMoon [43]

Answer:

All of the C-C bonds are actually identical,

The structure of the molecule is closed like a ring structure,

Explanation:

1) all benzene hydrocarbons are ChHp-2 ⇔ this is false the formula for benzene is C6H6 ( CnHn).

2)All C-C bonds share 2 pairs of electrons ⇔ False

There are not enough electrons to form double bonds on all the carbon atoms

3) Three C-C bonds share 2 pairs of electrons ⇔ False

Since there are not enough electrons to form double bonds on all the carbon atoms, although the electrons do strengthen all of the bonds on the ring equally.

4) All of the C-C bonds are actually identical ⇔ correct

⇒The actual structure of benzene is a resonance hybrid, with six delocalised π-electrons. (4n + 2 = π)

⇒Due to this structure with delocalised π-electrons, the structure of benzene is very stable and it's reactivity quite low.

⇒ All the C-C bonds of bezene have sp2-sp2 overlap on both sides, what makes them to form 3 π-bonds

5) The structure of the molecule is closed like a ring structure ⇔ correct

Since there are not enough electrons to form double bonds on all the carbon atoms, although the electrons do strengthen all of the bonds on the ring equally. This results in symmetric molecular orbital. The delocalisation of the electrons is also known as aromaticity or ring structure, what gives benzene a great stability.

3 0

2 years ago

15. An apparatus consists of a 4.0 dm3

Solnce55 [7]

Answer:

i· Partial pressure of nitrogen gas is 219.429kPa and partial pressure of argon gas is 33.714kPa ·

ii· Total pressure of the gas mixture is 253.143kPa·

Explanation:

<h3>solution for i :</h3>

Assuming that the given gases to be ideal,

so by ideal gas equation

PV=nRT

where,

P is the pressure of the gas

V is the volume occupied by the gas

n is the number of moles of the gas

R is the ideal gas constant

T is the temperature of the gas

Actually partial pressure of each gas is the pressure of the gas exerted when it occupies complete volume

As the temperature of both gases are same, the mixing process is an isothermal process

PV=constant

Initially for nitrogen gas PV=803×4=3212

let P $x_{1}$ be the partial pressure of the nitrogen gas

(P $x_{1}$ )×14=3212

∴P $x_{1}$ =219.429kPa

∴Partial pressure of nitrogen gas is 219.429kPa

Initially for argon gas PV=47.2×10=472

let P $x_{2}$ be the partial pressure of the argon gas

(P $x_{2}$ )×14=472

∴P $x_{2}$ =33.714kPa

∴Partial pressure of argon gas is 33.714kPa

solution for ii :

Total pressure of the gas mixture will be the sum of the partial pressures of each gas as

Partial pressure of the gas=(total pressure of the mixture)×(mole fraction of the gas)

∴Total pressure=P $x_{1}$ +P $x_{2}$

=219.429+33.719

Total pressure =253.143kPa

6 0

2 years ago

Read 2 more answers

The concentration of sugar in a soft drink is measured to be 10.5%. how many grams of sugar are in 125 g of the drink?

viva [34]

The grams of the sugar in 125 g of the drink is calculated as below

%M/m) = mass of the solute (sugar)/ mass of the solvent(drink) x100

let the mass of the solute(sugar) be represented by y

convert % into fraction by dividing by 100 = 10.5/100

10.5/100 = y/125

by cross multiplication

100y =1312.5
divide both side by 100

y=13.125 grams

5 0

2 years ago

If 16.0 mL of acetone is dissolved in water to make 155 mL of solution what is the concentration expressed in volume/volume % of

Lady_Fox [76]

Percentage by volume of solution is the percentage volume of solute in total volume of solution.
Volume percentage (v/v%) = volume of solute / total volume of solution x 100%
volume of solute - 16.0 mL
total volume of solution - 155 mL
v/v% = 16.0 / 155 x 100% = 10.32%
this means that in a volume of 100 mL solution, 10.32 mL is acetone.

7 0

2 years ago