Answer:
The sand bath spreads the heat out so that the flask is heated evenly. This reduces the chance of the flask breaking and ensures that there are no hot spots in the reaction mixture which could lead to excessive charring,
Explanation:
<span>a) molecular, phosphorous pentafluoride
b) ionic, sodium iodide
c) molecular, sulfur dichloride
d) ionic, calcium nitrate
e) ionic, iron(III) chloride
f) ionic?, lanthanum phosphate
g) ionic, cobalt(II) carbonate
h) molecular, dinitrogen tetraoxide
hope this helps!</span><span>
</span>
<h3>
Answer:</h3>
70.906 g
<h3>
Explanation:</h3>
We are given;
- Atoms of Chlorine = 1.2 × 10^24 atoms
We are required to calculate the mass of Chlorine
- We know that 1 mole of an element contains atoms equivalent to the Avogadro's number, 6.022 × 10^23.
- That is , 1 mole of an element = 6.022 × 10^23 atoms
- Therefore; 1 mole of Chlorine = 6.022 × 10^23 atoms
But since Chlorine gas is a molecule;
- 1 mole of Chlorine gas = 2 × 6.022 × 10^23 atoms
But, molar mass of Chlorine gas = 70.906 g/mol
Then;
70.906 g Of chlorine gas = 2 × 6.022 × 10^23 atoms
= 1.20 × 10^24 atoms
Thus;
For 1.2 × 10^24 atoms ;
= ( 70.906 g/mol × 1.2 × 10^24 atoms ) ÷ (1.20 × 10^24 atoms)
<h3>= 70.906 g </h3>
Therefore, 1.20 × 10^24 atoms of chlorine contains a mass of 70.906 g
=
Answer:
B : Their constant motion
C: Ideal gas law
Explanation:
Question 1:
Gas particles collides with the walls of their containers due to their constant motion.
Gases moves randomly and haphazardly in all direction and they collide with themselves and the walls of their container.
The kinetic theory of gases provides a better oversight into this;
- The pressure of the gases is caused by the frequent collision between the gases and their container.
- The molecules of gases collides with one another and with walls of their container elastically without any loss of kinetic energy.
Based on this premise, we can clearly decipher that gas particles collides with the walls of their containers because they are always in constant motion
Question 2:
Given parameters:
Mass of the Helium gas = 5g
Volume of gas = 10mL
Pressure on gas = 20mmHg
Unknown:
Appropriate gas law to solve this problem = ?
Solution:
The ideal gas law would be the perfect plug to derive the unknown temperature.
This gas law is a derivative of the of three gas laws which are;
- Boyle's law
- Charles's law
- Avogadro's law
The law is written as:
PV = nRT
P is the pressure
V is the volume
R is the gas constant
n is the number of moles
T is the unknown temperature in this problem
- The ideal gas law is used to find any of the variables (P, V, n and T)
the number of moles is;
number of moles =
Answer:
The correct answer is 0.75 atm
Explanation:
We have carbon monoxide gas (CO) at the following conditions:
T= 30ºC = 303 K
V= 20.0 L
m = 17 g
The molecular weight of CO (MM CO) is the following:
MM CO= molar mass of C + molar mass of O = 12 g/mol + 16 g/mol = 28 g/mol
We calculate the number of moles (n) as follows:
n= m/MM CO = 17 g/28 g/mol = 0.61 mol
Finally we use the ideal gases equation to calculate the pressure (P):
P x V = n x R x T
P = (n x R x T)/V
P= (0.61 mol x 0.082 L.atm/K.mol x 303 K)/20.0 L
P= 0.75 atm