Chemistry High School

The density of aluminum is 2.7 grams per cm'.
How many grams does 12 cm of aluminum
weigh?

Answers

Answer 1

Answer:

32.4grams

Explanation:

Density of a substance can be calculated as follows:

Density = mass ÷ volume

According to this question, the density of aluminum is 2.7g/cm³ while its volume is 12 cm³. The mass of aluminum is therefore,

2.7 = m/12

m = 12 × 2.7

m = 32.4grams.

The mass of aluminum is 32.4grams

Related Questions

What is the percent by mass of chlorine CI in NaCI to 3 significat digits please help

Answers

Answer:

60.7%

Explanation:

Molar mass of NaCl = 23 +35.5

= 58.5 g/mol

Molar mass of Cl = 35.5 g/mol

Percentage by mass of Cl =?

The percentage by mass of Cl in NaCl can be obtained as shown below'

Percentage by mass = mass of element / mass of the compound × 100

Percentage by mass of Cl

= 35.5 / 58.5 × 100

= 3550 / 58.5

= 60.7%

Therefore, the percentage by mass of Cl in NaCl is 60.7%

What type of molecule is 3-hexyne?

Answers

The type of molecule in which 3-hexyne is grouped under is referred to an alkyne.

What is Alkyne?

This is an organic compound which has a triple bond. It falls under the group of hydrocarbons present on earth.

They are usually represented with the suffix -yne which is why 3-hexyne falls under such category.

Read more about Alkyne here https://brainly.com/question/22933069

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A sample of gas occupies a volume of 55.3 L, has a temperature of 23.3 °C and a pressure of .658 atm. Calculate the number of moles of gas which are present in the sample. R= .0821 atm L/mol K

Answers

Answer: The number of moles of gas which are present in the sample are 1.49 mol.

Explanation:

Given: Volume = 55.3 L

Temperature = [tex]23.3^{o}C[/tex] = (23.3 + 273) K = 296.3 K

Pressure = 0.658 atm

Formula used is as follows.

PV = nRT

where,

P = pressure

V = volume

n = no. of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

[tex]PV = nRT\\0.658 atm \times 55.3 L = n \times 0.0821 L atm/mol K \times 296.3 K\\n = \frac{0.658 atm \times 55.3 L}{0.0821 L atm/mol K \times 296.3 K}\\= \frac{36.3874}{24.32623}\\= 1.49 mol[/tex]

Thus, we can conclude that the number of moles of gas which are present in the sample are 1.49 mol.

Cl2 + 2NO --> 2NOCI

What mass of NOCI will be produced if 2.58 X 10^22 molecules of CI2 react?

Answers

Answer:

Explanation:

Find the answer below

Can someone please solve this for me and explain it

Answers

83.3% yield

Explanation:

First, we need to convert 240 g of [tex]Fe_{2}O_{3}[/tex] into moles:

[tex]240 \:g \:Fe_{2}O_{3} \:\times(\frac{1\:\text{mol}\:Fe_{2}O_{3}}{159.69\: \text {g}\:Fe_{2}O_{3}})[/tex]

[tex]=1.50 \:\text{mol}\:Fe_{2}O_{3}[/tex]

Next, find the theoretical Fe yield using molar ratios.

[tex]1.50 \: \text {mol} \: Fe_{2}O_{3}\: \times (\frac{2\: \text{mol} \: Fe}{1 \:\text{mol} \: Fe_{2}O_{3}})[/tex]

[tex] = 3.00 \: \text{mol} \: Fe[/tex]

Then convert this back into grams:

[tex]3.00 \: \text{mol} \:Fe \times (\frac{55.845 \: \text{g} \: Fe}{1 \: \text{mol} \: Fe}) = 168 \: \text{g} \: Fe[/tex]

Note that actual yield is only 140 g Fe so percentage yield is

[tex]\dfrac{140\:\text{g}\:Fe}{168\:\text{g}\:Fe} \times 100[/tex]%= 83.3%

83.3%

The answer is 83.3%

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