Chemistry
Atoms and Atomic Structure
Molecular Mass

# What form of the ideal gas law would you use to calculate the number of moles?

This is the general law of gases:
PV = nRT (n is the number of moles)

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n=PV/RT

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## Related Questions

The formula is: pV=nRT where: - p is the pressure in at - V is the vome in L - R is the gas constant: 0,082057 - T is the temerature in kelvin - number of moles

Use the ideal gas law, PV=nRT. P= pressure V= volume n= number of moles R= gas law constant T= temperature If you have P, V, R, T then you can solve for "n" to find the number of moles. There are a number of ways and variations that you can go about finding the number of moles, but all would involve the ideal gas law or a similar formula.

Using the ideal gas law (using torr instead of atm), we calculate that there would be .046 moles of CO, or 2.7x1022 molecules of carbon monoxide.

The formula is: T = PV/nR, Where: * T is the temperature in kelvin * P is the pressure in atmospheres * n is the number of moles * R is the gas constant

The mass of 3 mol of ammonia is 51,093 g; the number of ammonia molecules in 3 moles is18,066422571.10e23.

58,44 is the molecular weight of NaCl. So 15/58,44 = 0.257 moles would be contained in 15 g.

1 mole of an ideal gas occupies 22.4 liters at STP. So 112 liters would be occupied by 5 moles of an ideal gas.

we have to calculate number of moles in 8gram of oxygen by the equation given mass/molar mass.then we would get that 0.25moles are in 8 g of oxygen molecules.then multiply this to avagadro number .then we could get the number of particles.

This number is the Avogadro number: 6,02214129(27)&Atilde;&mdash;1023 mol&acirc;&circ;&rsquo;1. For the measurement see the link below.

Assuming that you are trying to find the number of moles in an elemental sample, you would take the mass of the sample, and divide by the atomic weight of the substance. This will give you the number of atoms. You this divide this by Avogadro's number (6.0221415 x 1023). This will give you the number of moles in the sample. I even saw a mole once, but it was chased under the porch by a cation. &#9632;

The number of grams in 4.56 moles of H2O2 would be 7.57. This is a math problem.

The number of moles of solute dissolved in 1 L of a solution would be the molarity. As an example, if you had 2 moles of solute in 1 liter the molarity would be 2M.

Knowing what the answer options are is important for a person to know which is correct. It would be helpful to provide the answer choices as well.

The number 2.20 moles converted in Sn would be 2161.14. This is taugh in biology.

In order to convert you would need to multiply the number of moles by Avogadro's number (6.022 x 1023). And that would give you atoms (or molecules or ions).

The answer to this question lies in the ideal gas law: PV=nrT in which: P = presssure V = Volume n = number of moles r = ideal gas constant T = temperature because we want P to increase, we can achieve that in a couple of ways: 1. decrease the volume 2. increase the number of moles 3. increase the temperature. Value of r cannot change; it is a constant.

The mass of 5 mol of ammonia is 85,155 g; the number of ammonia molecules in 5 moles is3,011 070 428 5.10e24.

number of moles = mass of the element/molar mass of the element

You have to multiply the number of moles by Avogadro's number (6.022x10^23). The product of the two numbers will give you the number of atoms.

Number of moles = mass of the sample/atomic weight of Al = 96,7/26,987 = 3,58

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