The density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
<h3>What is the
Ideal Gas Law ?</h3>
This law combines the relationships between p, V, T and mass, and gives a number to the constant.
The ideal gas law is:
pV = nRT
where n is the number of moles, and R is universal gas constant.
The value of R depends on the units involved, but is usually stated with S.I. units as: R = 8.314 J/mol·K
The values given in the question are
p= 5.30 atm , V=3.50 L
T (in Kelvin) = 125+273 K
= 398 K
R = 0.0821 L·atm /mol·K
The Ideal Gas equation can be re written as
pM=DRT
M is the molar mass , D is the density
M for N₂ is 28 gm/mol
so density can be determined as
Therefore the density of a sample of nitrogen gas (N₂) that exerts a pressure of 5.30 atm in a 3.50-L container at 125°C is 4.54 gm/litre
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Hey there!
Exothermic reactions release heat, causing its temperature to fall. If the reaction is lessening the temperature of the object while releasing all the heat, then you know that the reaction is indeed exothermic. Hope this helps!
Answer:
N
Explanation:
Electronegativity increases as you move from left to right across a period, and decreases as you move down the groups.
There are 500 mg of calcium carbonate is in this caltrate tablet
The equation of the reaction is;
2HCl(aq) + CaCO3(aq) ------> CaCl2(aq) + CO2(g) + H2O(l)
Next, we have to obtain the amount HCl reacted as follows;
Number of moles = concentration × volume
Volume = 34.46 mL or 0.03446 L
Concentration = 0.291 M
Number of moles = 0.291 M × 0.03446 L
Number of moles = 0.01 moles
Since the reaction of HCl and CaCO3 are in the ratio of 2:1
2 moles of HCl reacts with 1 mole of CaCO3
0.01 moles of HCl reacts with 0.01 moles × 1 mole/2 moles
= 0.005 moles of CaCO3
Mass of CaCO3 = number of moles × molar mass
Mass of CaCO3 = 0.005 moles of CaCO3 × 100 g/mol
Mass of CaCO3 = 0.5 g or 500 mg
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