What volume will 2.04g of helium gas occupy at 100C and 1.13 atm?

A volume measured by a graduated cylinder that was marked in 100 mL

Natali [406]

The volume measured using such a cylinder will be reported to the nearest 10th mL.

<h3>Cylinder graduation</h3>

10 mL graduated cylinders are always read to the nearest two decimal places.

100 mL graduated cylinders are always read to the nearest 1 decimal place. The nearest 1 decimal place is the same thing as the nearest 10th.

Thus, a reading made using a 100mL increment graduated cylinder would be reported to the nearest 10th mL.

More on cylinder graduation can be found here: brainly.com/question/14427988

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8 0

2 years ago

How is heat produced in a chemical change

Snezhnost [94]

Answer:Hola UwU

Most chemical reactions involve the breaking and formation of chemical bonds. It takes energy to break a chemical bond but energy is released when chemical bonds are formed. If more energy is released than consumed, then the chemical reaction evolves heat and is said to be exothermic.

Explanation:Adios~ UnU haha

7 0

3 years ago

Its gelatin and a fruit cup the same (its for a project)

gizmo_the_mogwai [7]

Answer:

No

Explanation:

Gelatin is a substance that makes jello, and a fruit cup is a cup full of fruit

6 0

3 years ago

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Answer these questions based on 234.04360 as the atomic mass of thorium-234. The masses for the subatomic particles are given. R

Scilla [17]

How many protons does Thorium have? 90

How many neutrons does Thorium-234 have? 144

Calculate the mass defect for the isotope thorium-234 1.85864 amu

4 0

4 years ago

Read 2 more answers

mixture of N 2 And H2 Gases weighs 13.22 g and occupies a volume of 24.62 L at 300 K and 1.00 atm.Calculate the mass percent of

anygoal [31]

Answer: The mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

Explanation:

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

PV = nRT

where,

P = Pressure of the gaseous mixture = 1.00 atm

V = Volume of the gaseous mixture = 24.62 L

n = number of moles of the gaseous mixture = ?

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

T = Temperature of the gaseous mixture = 300 K

Putting values in above equation, we get:

$1.00atm\times 24.62L=n_{mix}\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 300K\\\\n_{mix}=\frac{1.00\times 24.62}{0.0821\times 300}=0.9996mol$

We are given:

Total mass of the mixture = 13.22 grams

Let the mass of nitrogen gas be 'x' grams and that of hydrogen gas be '(13.22 - x)' grams

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

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

For nitrogen gas:

Molar mass of nitrogen gas = 28 g/mol

$\text{Moles of nitrogen gas}=\frac{x}{28}mol$

For hydrogen gas:

Molar mass of hydrogen gas = 2 g/mol

$\text{Moles of hydrogen gas}=\frac{(13.22-x)}{2}mol$

Equating the moles of the individual gases to the moles of mixture:

$0.9996=\frac{x}{28}+\frac{(13.22-x)}{2}\\\\x=12.084g$

To calculate the mass percentage of substance in mixture we use the equation:

$\text{Mass percent of substance}=\frac{\text{Mass of substance}}{\text{Mass of mixture}}\times 100$

Mass of the mixture = 13.22 g

For nitrogen gas:

Mass of nitrogen gas = x = 12.084 g

Putting values in above equation, we get:

$\text{Mass percent of nitrogen gas}=\frac{12.084g}{13.22g}\times 100=91.41\%$

For hydrogen gas:

Mass of hydrogen gas = (13.22 - x) = (13.22 - 12.084) g = 1.136 g

Putting values in above equation, we get:

$\text{Mass percent of hydrogen gas}=\frac{1.136g}{13.22g}\times 100=8.59\%$

Hence, the mass percent of nitrogen gas and hydrogen gas is 91.41 % and 8.59 % respectively.

5 0

3 years ago