Answer:
3.97 x 10²² molecules
Explanation:
To find the moles, you need to use the Ideal Gas Law:
PV = nRT
In this equation,
-----> P = pressure (atm)
-----> V = volume (L)
-----> n = moles
-----> R = Ideal Gas constant (0.08206 atm*L/mol*K)
-----> T = temperature (K)
Before you can plug the values into the equation, you need to (1) convert the pressure from torr to atm (by dividing by 760), then (2) convert the volume from mL to L (by dividing by 1000), and then (3) convert the temperature from Celsius to Kelvin (by adding 273).
P = 800.0 torr / 760 = 1.05 atm R = 0.08206 atm*L/mol*K
V = 1500 mL / 1000 = 1.5 L T = 19.0 °C + 273 = 292 K
n = ? moles
PV = nRT
(1.05 atm)(1.5 L) = n(0.08206 atm*L/mol*K)(292 K)
1.579 = n(23.96)
0.0659 = moles
Now, you need to convert moles to molecules using Avogadro's Number.
Avogadro's Number:
6.022 x 10²³ molecules = 1 mole
0.0659 moles 6.022 x 10²³ molecules
------------------------ x ------------------------------------- = 3.97 x 10²² molecules
1 mole
For the reactants,
- The oxidation number of hydrogen = +1
- The oxidation number of oxygen = -2
- The oxidation number of arsenic = +5
- The oxidation number of carbon = +3
For the products,
- The oxidation number of hydrogen = +1
- The oxidation number of oxygen = -2
- The oxidation number of arsenic = +3
- The oxidation number of carbon = +4
Here, arsenic (+5 to +3) and carbon (+3 to +4) are the only oxidation numbers changing.
Note that an increase in oxidation number means electrons are lost. Thus oxidation is occurring, and a decrease in oxidation number means electrons are being gained, and thus reduction is occurring.
Also, the compound that contains the element being oxidized is the reducing agent, and the compound that contains the element being reduced is the oxidizing agent.
So, the answers are:
name of the element oxidized: Carbon
name of the element reduced: Arsenic
formula of the oxidizing agent:
formula of the reducing agent:
Heat is require for a high number of collisions.