Density = mass / volume
Since the answer must be in g/ml
Convert volume to ml
0.1266 x 1000 = 126.6 ml
15.196 / 126.6
= 0.126 g/ml
T₁ = 27°C = 27 + 273 = 300K, V₁ = 6 L,
T₂ = 150°C = 150 + 273 = 423K, V₂ = ?,
By Charles' Law: V₁/T₁= V₂/T₂
6/300 = V₂/423
423*(6/300) = V₂
8.46 = V₂
Volume at 150°C =8.46 L.
Answer:
8,19 L
Explanation:
The combined gas law is a equation that can be used <em>when the initial and final conditions -</em>pressure,volume,amount of moles,temperature-, <em>of a gas change</em> during a process. It can be written:
If the amount of the gas remains constant, then n1=n2 and we have:
For the problem we have:
<em>Note: When working with gases is important to use </em><em><u>absolute temperature values (°K, °K=°C+273,15):</u></em>
P1=1 atm, V1=2,5L, T1=25+273,15=298,15°K
P2=0,3 atm, V2=?, T2=20+273,15=293,15°K
The new volume of the balloon is 8,19 L.
The answer is (a) 30g. Zinc = 30. 1 mole = 30 x 1 = 30g
Answer:
I. The balloon has a volume of 22.4L
III. The balloon contains 6.022x10^23 molecules.
Explanation:
At stp, it has been proven that 1mole of a gas occupy 22.4L.
Therefore, option (i) is correct.
The molar mass N2 = 14.01 x 2 = 28.02g/mol
Number of mole of N2 = 1 mole
Mass of N2 =..?
Mass = mole x molar Mass
Mass of N2 = 1 x 28.02 = 28.02g.
The mass content of the balloon is 28.02g, therefore, option (ii) is wrong.
From Avogadro's hypothesis, we understood that 1 mole of any substance contains 6.02x10^23 molecules. This implies that 1 mole of N2 also contains 6.02x10^23 molecules
Therefore, option (iii) is correct.
The correct options to the question are:
Option i and option iii
