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2 years ago

What volume is equivalent to 0.0015 m3?

Chemistry

1 answer:

vaieri [72.5K]2 years ago

3 0

Answer : Option 'D' is correct.

$0.0015m^{3}$ = $1.5\times 10^{6}mm^{3}$

Explanation 1) : 1 m = 100 cm

$1 m^{3}= 1000000 cm^{3}$ or $1 m^{3}= 10^{6} cm^{3}$

$(0.0015m^{3})\times \frac{(1000000cm^{3})}{(1m^{3})}$

$(0.0015)\times \frac{(1000000cm^{3})}{(1)}$ = $1500cm^{3}$

$0.0015m^{3}$ = $1500cm^{3}$ = $1.5\times 10^{3}cm^{3}$

Explanation 2) : 1 m = 1000 mm

$1m^{3}= 1000000000mm^{3} = 10^{9}mm^{3}$

$(0.0015m^{3})\times \frac{(10^{9}mm^{3})}{(1m^{3})}$

$(0.0015)\times \frac{(10^{9}mm^{3})}{(1)}$ = $1500000 mm^{3}$

$0.0015m^{3}$ = $1500000 mm^{3}$ = $1.5\times 10^{6}mm^{3}$

Option 'D' is right.

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A solution is prepared by dissolving 91.7 g fructose in 545 g of water. Determine the mole fraction of fructose if the final vol

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Answer:

Mole fraction = 0,0166

Explanation:

Mole fraction is defined as mole of a compound per total moles of the mixture. In the solution, the solute is fructose and the solvent is water. That means you need to find moles of fructose and moles of water.

The molecular mass of fructose is 180,16g/mol and mass of water is 18,02 g/mol. Using these values:

91,7g fructose × (1mol / 180,16g) = 0,509 moles of fructose

545g water × (1mol / 18,02g) = 30,24 moles of water

Thus, mole fraction of fructose is:

$\frac{0,509 moles}{0,509mol + 30,24mol} = 0,0166$

Mole fraction = 0,0166

I hope it helps!

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2 years ago

You are given three bottles labeled a, b, and

ElenaW [278]

Answer :Solid in bottle a is ionic, solid in bottle b is molecular and solid in bottle c is ionic.

Explanation :

Ionic compound is formed when a metal atom donates one or more electrons to a non metal. This results in the formation of a cation ( a positive ion) and an anion ( a negative ion). These ions are bonded to each other by electrostatic attraction.

The intermolecular forces in case of a an ionic compound are very strong.

The melting point of a substance depends on how strongly the molecules are attracted to each other. Stronger the forces, higher is the melting point.

Therefore ionic compounds always have very high melting points.

On the other hand, covalent compounds have weak intermolecular forces. Therefore they have low melting points.

Based on above discussion, we can classify the given compounds as follows.

a) Solid in bottle a is Ionic as it has high melting point.

b) Solid in bottle b is molecular as it has low melting point.

c) Solid in bottle c is Ionic as it has high melting point.

6 0

2 years ago

How many grams of NH3 can be prepared from the synthesis of 77.3 grams of nitrogen and 14.2 grams of hydrogen gas?

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Answer:

80.41 g

Explanation:

Data Given:

Mass of Nitrogen (N₂) = 77.3 g

Mass of Hydrogen (H₂) = 14.2 g

many grams of NH₃ = ?

Solution:

First we look at the balanced synthesis reaction

N₂ + 3 H₂ ------—> 2 NH₃

1 mol 3 mol

As 1 mole of Nitrogen react with 3 mole of hydrogen

Convert moles to mass

molar mass of N₂ = 2(14) = 28 g/mol

molar mass of H₂ = 2(1) + 2 g/mol

Now

N₂ + 3 H₂ ------—> 2 NH₃

1 mol (28 g/mol) 3 mol(2g/mol)

28 g 6 g

28 grams of N₂ react with 6 g of H₂

if 28 grams of N₂ produces 6 g of H₂ so how many grams of N₂ will react with 14.2 g of H₂.

Apply Unity Formula

28 g of N₂ ≅ 6 g of H₂

X g of N₂ ≅ 14.2 g of H₂

Do cross multiply

X g of N₂ = 28 g x 14.2 g / 6 g

X g of N₂ = 66.3 g

As we have given with 77. 3 g of N₂ but from this calculation we come to know that 66.3 g will react with 14.2 g of hydrogen and the remaining 10 g N₂ will be in excess

So, Hydrogen is limiting reactant in this reaction and the amount of NH₃ depends on the amount of hydrogen.

Now

To find mass of NH₃ we will do following calculation

Look at the reaction

As we Know

N₂ + 3 H₂ ------—> 2 NH₃

6 g 2 mol

So, 6 g of hydrogen gives 2 moles of NH₃, then how many moles of NH₃ will be produce by 14.2 g

Apply Unity Formula

6 g of H₂ ≅ 2 mol of NH₃

14.2 g of H₂ ≅ X mol of NH₃

Do cross multiply

X mol of NH₃= 14.2 g x 2 mol / 6 g

X mol of NH₃ = 4.73 mol

So, 14.2 g of hydrogen gives 4.73 moles of NH₃

Now

Convert moles of NH₃ to mass

Formula will be used

mass in grams = no. of moles x molar mass . . . . . . (2)

Molar mass of NH₃

Molar mass of NH₃ = 14 + 3(1)

Molar mass of NH₃ = 14 + 3 = 17 g/mol

Put values in equation 2

mass in grams = 4.73 mole x 17 g/mol

mass in grams = 80.41 g

mass of NH₃= 80.41 g

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2 years ago

Olympic cyclist fill their tires with helium to make them lighter. Calculate the mass of air in an air filled tire and the mass

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Answer: The mass difference between the two is 7.38 grams.

Explanation:

To calculate the number of moles, we use the equation given by ideal gas follows:

$PV=nRT$

where,

P = pressure = 125 psi = 8.50 atm (Conversion factor: 1 atm = 14.7 psi)

V = Volume = 855 mL = 0.855 L (Conversion factor: 1 L = 1000 mL)

T = Temperature = $25^oC=[25+273]K=298K$

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

n = number of moles = ?

Putting values in above equation, we get:

$8.50atm\times 0.855L=n\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 298K\\\\n=\frac{8.50\times 0.855}{0.0821\times 298}=0.297mol$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For air:

Moles of air = 0.297 moles

Average molar mass of air = 28.8 g/mol

Putting values in equation 1, we get:

$0.297mol=\frac{\text{Mass of air}}{28.8g/mol}\\\\\text{Mass of air}=(0.297mol\times 28.8g/mol)=8.56g$

Mass of air, $m_1$ = 8.56 g

For helium gas:

Moles of helium = 0.297 moles

Molar mass of helium = 4 g/mol

Putting values in equation 1, we get:

$0.297mol=\frac{\text{Mass of helium}}{4g/mol}\\\\\text{Mass of helium}=(0.297mol\times 4g/mol)=1.18g$

Mass of helium, $m_2$ = 1.18 g

Calculating the mass difference between the two:

$\Delta m=m_1-m_2$

$\Delta m=(8.56-1.18)g=7.38g$

Hence, the mass difference between the two is 7.38 grams.

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2 years ago

In the reaction 2Li(s) + 2H2O(l) 2LiOH(aq) + H2(g), what compound is in the gaseous state?

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Answer is: C. H₂, molecule of hydrogen, g is chemistry abbreviations or physical state symbol for gas.

Lithium (Li) is solid (s) element (metal).
Water (H₂O) is liquid (l) compound or molecule.
Lithium hydroxide (LiOH) is aqueous solution (aq). It dissociates in water on lithium cation (Li⁺) and hydroxy anion (OH⁻).

6 0

2 years ago