Explanation:
I think there' will be a decrease in volume of the air.
Answer:
323.22 ml
Explanation:
Given that :
Diameter, d = 6.8cm
Height, h = 8.9cm
V = arh
Recall :
Volume, V = πr²h
Radius, r = diameter / 2 = 6.8 / 2 = 3.4cm
V = π * 3.4^2 * 8.9
V = 323.21961 cm³
Recall:
1ml = 1cm³
Hence,
323.21961 cm³ = 323.21961 ml
Volume = 323.22 ml
Stronger intermolecular forces = higher boiling point
The stronger the intermolecular forces, the harder the molecules are to pull/break apart, which means a higher boiling point.
Answer:
7.81 moles
Explanation:
To solve this problem, let us generate an expression involving volume and number of mole of the gas since the pressure and temperature of the gas are constant.
From ideal gas equation:
PV = nRT
Divide both side by P
V= nRT/P
Divide both side by n
V/n = RT/P
Since RT/P are constant, then:
V1/n1 = V2/n2
Data obtained from the question include:
V1 = 4.11
n1 = 2.51 moles
V2 = 16.9L
n2 =?
Using the above equation i.e V1/n1 = V2/n2, the final number of the gas can be obtained as illustrated below:
4.11/2.51 = 16.9/n2
Cross multiply to express in linear form
4.11 x n2 = 2.51 x 16.9
Divide both side by 4.11
n2 = (2.51 x 16.9) / 4.11
n2 = 10.32moles
Now, to obtain the number of mole of the gas added, we'll subtract the initial mole from the final mole i.e
n2 — n1
Number of mole added = n2 — n1
10.32 — 2.51 = 7.81 moles
Therefore, 7.81 moles of the gas was added to the container
Answer:
<h2>30.2 g</h2>
Explanation:
The mass of a substance when given the density and volume can be found by using the formula
mass = Density × volume
volume = final volume of water - initial volume of water
From the question
volume = 35.9 ml - 25.8 ml = 10.1 mL
We have
mass = 2.99 × 10.1 = 30.199 g
We have the final answer as
<h3>30.2 g</h3>
Hope this helps you
