How many significant figures are there in the number 3.04
2 answers:
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Answer:
Explanation:
Hello,
In this case, the undergoing chemical reaction is:
Next, we identify the limiting reactant by computing the moles of magnesium oxide yielded by 3.86 g of magnesium and 155 mL of oxygen at the given conditions via their 2:1:2 mole ratios and the ideal gas equation:
It means that the limiting reactant is the oxygen as it yields the smallest amount of magnesium oxide. Next, we compute the mass of magnesium consumed the oxygen only:
Thus, the mass in excess is:
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Answer:
i· Partial pressure of nitrogen gas is 219.429kPa and partial pressure of argon gas is 33.714kPa ·
ii· Total pressure of the gas mixture is 253.143kPa·
Explanation:
<h3>solution for i :</h3>Assuming that the given gases to be ideal,
so by ideal gas equation
PV=nRT
where,
P is the pressure of the gas
V is the volume occupied by the gas
n is the number of moles of the gas
R is the ideal gas constant
T is the temperature of the gas
Actually partial pressure of each gas is the pressure of the gas exerted when it occupies complete volume
As the temperature of both gases are same, the mixing process is an isothermal process
PV=constant
Initially for nitrogen gas PV=803×4=3212
let P be the partial pressure of the nitrogen gas
(P)×14=3212
∴P=219.429kPa
∴Partial pressure of nitrogen gas is 219.429kPa
Initially for argon gas PV=47.2×10=472
let P be the partial pressure of the argon gas
(P)×14=472
∴P=33.714kPa
∴Partial pressure of argon gas is 33.714kPa
solution for ii :
Total pressure of the gas mixture will be the sum of the partial pressures of each gas as
Partial pressure of the gas=(total pressure of the mixture)×(mole fraction of the gas)
∴Total pressure=P+P
=219.429+33.719
Total pressure =253.143kPa