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DaniilM [7]
3 years ago
13

What is the mass, in grams, of 6.11 mol of sulfur trioxide?

Chemistry
2 answers:
Travka [436]3 years ago
8 0

Answer : The mass of sulfur trioxide is, 488.8 grams.

Explanation : Given,

Moles of sulfur trioxide = 6.11 mole

Molar mass of sulfur trioxide = 80 g/mole

Formula used :

\text{Mass of }SO_3=\text{Moles of }SO_3\times \text{Molar mass of }SO_3

Now put all the given values in this formula, we get the mass of sulfur trioxide.

\text{Mass of }SO_3=6.11mole\times 80g/mole=488.8g

Therefore, the mass of sulfur trioxide is, 488.8 grams.

Kazeer [188]3 years ago
7 0
It would be approximately 489 g, rounded for significant figures. The calculator given answer would be 489.20326. To get that, all you have to do is take your 6.11 moles and multiply it by 80.066 (the molar mass) divided by 1 mol to cancel out the unit. 
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Pete Gannett

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Ph.D. Chemistry, University of Wisconsin-Madison, (1982)2y

Seems to be an ideal gas law question. The relevant equation is:

PV = nRT

where P is the pressure in atmospheres, V is the volume in liters, n is the number of moles of gas, R is the gas constant (0.082 atm-L/mole-deg K), and T is temperature in Kelvins. STP means standard temperature and pressure and this is taken as 1 atm and 0º C or 273 K.

To calculate the number of molecules we will use the constant 6.023 * 10^23 molecules/mole and, therefore, we will need to know the number of moles (n). So, first we’ll rearrange the gas law equation, isolating ’n’ and then put the numbers in.

n = PV/RT = 1 * 1 / (0.082)(273) = 0.0447 moles

So, to calculate the number of molecules, multiple this by the number of molecules in a mole and you get:

# molecules of nitrogen in 1 Liter at STP = 6.023 * 10^23 molecules/mole * 0.0447 moles = 2.6905 * 10^22 molecules

Note, it does not matter what the gas is.

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