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2 years ago

A sample of carbon monoxide and oxygen gasses are

Chemistry

1 answer:

otez555 [7]2 years ago

3 0

Answer:

.0172 mole of CO2

Explanation:

PV = nR T n = number of moles V = .5 liter

R = gas constant = .082057 L atm/(k mole)

T needs to be in Kelvin = C + 273.15

.868 * .5 = n * .082057 * ( 35 + 273.15)

n = .0172 moles

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Within the nuclear us of individual Adams of the same element, the proton number

AnnyKZ [126]

the same

Explanation:

Within the nucleus of individual atoms of the same element, the proton number is the same.

All atoms of the same kind from the same element have the same number of protons.

The number of protons does not change, it remains fixed after a chemical reaction.

Different elements have different number of protons that typifies and makes them unique.

But atoms of the same element have the same number of protons in them.

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Atomic number brainly.com/question/5425825

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4 years ago

Andrews [41]

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3 years ago

True or False- The parts of a mixture keep their own properties when they are combined.

ICE Princess25 [194]

It is true yes :) happy to help

4 0

3 years ago

Investigate: Note the empty jars on the shelf that can be filled by using the slider. Set the amount to 2.000 moles of carbon (m

balandron [24]

Answer:

The molar mass of carbon

Explanation:

Before the mass (in grams) of two moles of carbon can be determined, the molar mass of the element would be needed.

This is because the number of mole of an element is the ratio of its mass and the molar mass. That is,

number of mole = mass/molar mass

Hence, the mass of elements can be obtained by making it the subject of the formular;

mass = number of mole x molar mass

Therefore, the molar mass of carbon would be needed before the mass of 2 moles of the element can be determined.

3 0

3 years ago

A steel container with a movable piston contains 2.00 g of helium which was held at a constant temperature of 25 °C. Additional

shtirl [24]

Answer: D) 1.00 g

Explanation:

According to the Avogadro's law, the volume of gas is directly proportional to the number of moles of gas at same pressure and temperature. That means,

$V\propto n$

or,

$\frac{V_1}{V_2}=\frac{n_1}{n_2}$

where,

$V_1$ = initial volume of gas = 2.00 L

$V_2$ = final volume of gas = 3.00 L

$n_1$ = initial moles of gas = $\frac{\text {Given mass of helium}}{\text {molar mass of helium}}=\frac{2.00g}{4g/mol}=0.500mol$

$n_2$ = final moles of gas = ?

Now we put all the given values in this formula, we get

$\frac{2.00L}{3.00L}=\frac{0.500mol}{n_2}$

$n_2=0.75mole$

Mass of helium = $moles\times {\text {molar mass}}=0.75\times 4=3.00g$

Thus mass of helium added = (3.00-2.00) g = 1.00 g

4 0

3 years ago