First convert each mass to moles by dividing by the molar mass.
0.347g Oxygen = 0.022 moles
0.260g Carbon = 0.022 moles
1.537g Chlorine = 0.043 moles
Divide each by smallest mole vale (0.022)
Oxygen = 0.022/0.022 = 1
Carbon = 0.022/0.022 = 1
Chlorine = 0.043/0.022 = 2
Therefore the empirical formula is COCl2
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Lets name one gas sample as A and other gas sample as B.
we can apply ideal gas law equation for both samples
PV = nRT
P - Pressure of A = Pressure of B
V - volume of A = volume of B
n - number of molecules of both A and B being equal is equivalent to number of moles of A = number of moles of B
R - universal gas constant
Tᵃ - temperature of A
Tᵇ - temperature of B
for gas A
PV = nRTᵃ --1)
for gas B
PV = nRTᵇ ---2)
when we divide both equations
1 = Tᵃ / Tᵇ
Tᵃ = Tᵇ
both temperatures are equal
temperature in Celsius + 273 = temperature in Kelvin
therefore 0 °C = 273 K
the correct answer is
A)
<span>The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0 </span>°<span>C</span>
Answer:
option C is correct
Explanation:
oxidation number is the apparent charge on an atom which it acquire after lose or gain of electron
Answer: about 1,705,536 hrs
24 hrs = 1 day
189 hrs = 1 week
756 = 1 month
9072 = 1 yr
1,705,536 = 188 yrs
Explanation:
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