Use the ideal gas law to calculate the pressure in atmospheres of 0.21 mol of helium (He) at 16°C & occupying 2.53 L. You mu
st show all of your work to earn credit. **Don't forget to convert your Celsius temperature to Kelvin**
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<u>Answer:</u> The mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.
<u>Explanation:</u>
To calculate the number of moles, we use the equation:
.....(1)
- <u>For nickel:</u>
Given mass of nickel = 14.8 g
Molar mass of nickel = 58.7 g/mol
Putting values in equation 1, we get:
For the given chemical reaction:
- <u>For nickel (II) oxide:</u>
By Stoichiometry of the reaction:
3 moles of nickel are produced from 3 moles of nickel (II) oxide
So, 0.252 moles of nickel will be produced from of nickel (II) oxide
Now, calculating the mass of nickel (II) oxide by using equation 1:
Molar mass of nickel (II) oxide = 74.7 g/mol
Moles of nickel (II) oxide = 0.252 moles
Putting values in equation 1, we get:
- <u>For aluminium:</u>
By Stoichiometry of the reaction:
3 moles of nickel are produced from 2 moles of aluminium
So, 0.252 moles of nickel will be produced from of aluminium
Now, calculating the mass of aluminium by using equation 1:
Molar mass of aluminium = 27 g/mol
Moles of aluminium = 0.168 moles
Putting values in equation 1, we get:
Hence, the mass of nickel (II) oxide and aluminium that must be used is 18.8 g and 4.54 g respectively.
Answer: 24.1 L
Explanation:
To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.
Mathematically,
where,
are the initial volume and temperature of the gas.
are the final volume and temperature of the gas.
We are given:
Putting values in above equation, we get:
Thus the volume of the sample when heated to 220.0oC and the pressure is constant is 24.1 L