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3 years ago

How many moles is 22.4 liters of oxygen gas at standard temperature and pressure represent

Chemistry

1 answer:

makkiz [27]3 years ago

7 0

Answer:

So 1 mole

Explanation:

PV = nRT

P = Pressure atm

V = Volume L

n = Moles

R = 0.08206 L·atm·mol−1·K−1.

T = Temperature K

standard temperature = 273K

standard pressure = 1 atm

22.4 liters of oxygen

Ok so we have

V = 22.4

P = 1 atm

PV = nRT

n = PV/RT

n = 22.4/(0.08206 x 273)

n = 22.4/22.40

n = 1 mole

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How can I calculate the mass percent of carbon, nitrogen and oxygen in caffeine, C8H10N4O2.

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You must first calculate the total weight of 1 mole of the substance. You do this by finding the molar weights on the periodic table of each of the elements in the compound:

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8 0

3 years ago

Read 2 more answers

A sample of a compound that contains only the elements C, H, and N is completely burned in O2 to produce 44.0 g of CO2, 45.0 g o

PolarNik [594]

Explanation:

what you have to do is to multiply the given grams with the ratio of grams of that certain element in it's full compound in order to isolate the compound and get the element.

because the question did not specify how many grams of NO2 is formed, we can assume that the mass is neglegible, thus 1 mole was assigned to Nitrogen.