Answer:
moles O₂ needed = 0.19 mole
Explanation:
4Fe(s) + 3O₂(g) => 2Fe₂O₃(s)
1.396g Fe(s) = 1.396g/56g/mol = 0.025 mole Fe(s)
0.025 mole Fe(s) reacts with 3/4(0.025 mole O₂(g) = 0.019 mole O₂(g)
<h3>
Answer:</h3>
Partial pressure of He(P(He) = 1.5 atm.
Partial pressure of Ne(P(Ne) = 1 atm.
Partial pressure of Ar(P(Ar) = 0.5 atm.
<h3>
Explanation:</h3>
According to Dalton law of partial pressure the sum of partial pressures of individual gases in a gaseous mixture is equivalent to the total pressure.
The partial pressure of a gas in a gaseous mixture is given by the product of the mole fraction and the total pressure.
Our gaseous mixture contains He, Ne, and Ar and the total pressure is 3 atm.
Since we are given the ratios of the gases in the mixture, we can calculate the partial pressure of each gas.
P(He) = 3/6 × 3 atm.
= 1.5 atm.
P(Ne) = 2/6 × 3 atm.
= 1 atm
P(Ar) = 1/6 × 3 atm.
= 0.5 atm
Therefore, the partial pressures of gases He, Ne and Ar are 1.5 atm, 1 atm, and 0.5 atm respectively.
In a combustion reaction, one of the reactants is always oxygen.
Answer:
Explanation:
Range = Highest value - Lowest value
A 'soft solder' melts between 183 °C and 212 °C.
Melting range of a 'soft solder' = 
A 'hard solder' melts between 620 °C and 680 °C.
Melting range of a 'hard solder' = 
So,
Difference in melting ranges = Melting range of a 'hard solder' - Melting range of a 'soft solder' = 
