Answer:
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Answer:
Partial pressure of O₂ = 0.0198 atm
Partial pressure of He = 0.1584 atm
Explanation:
Given data:
Mass of oxygen = 80.0 g
Mass of helium = 80.0 g
Total pressure = 0.1800 atm
Partial pressure of each gas = ?
Solution:
First of all we will calculate the number of moles.
Number of moles of oxygen:
Number of moles = mass/molar mass
Number of moles = 80.0 g/ 32 g/mol
Number of moles = 2.5 mol
Number of moles of helium:
Number of moles = mass/molar mass
Number of moles = 80.0 g/ 4 g/mol
Number of moles = 20 mol
Total number of moles = 20 mol + 2.5 mol = 22.5 mol
Mole fraction of O₂ = 2.5 mol/ 22.5 mol = 0.11
Mole fraction of He = 20 mol / 22.5 mol = 0.88
Partial pressure:
Partial pressure of O₂ = 0.11× 0.1800 atm = 0.0198 atm
Partial pressure of He = 0.88 × 0.1800 atm = 0.1584 atm
Answer:
P = 34.1 L
Explanation:
Given data:
Number of moles = 10 mol
Volume occupy = 15 L
Temperature = 350°C
Pressure of gas = ?
Solution:
The given problem will be solve by using general gas equation,
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
Now we will convert the temperature.
350+273 = 623 K
by putting values,
P×15 L = 10 mol ×0.0821 atm.L/ mol.K ×623 K
P = 511.48atm.L/15L
P = 34.1 L
Answer:
Mg(s) + 2HCl(aq) → MgCl2(s) + H2(g)
Explanation:
Many metal undergo displacement reaction . The most reactive metal will displace the less reactive metal from it compound. A single displacement reaction is a reaction in which one element displaces another in it compound.
Many metal undergo displacement reaction with hydrogen chloride . One example is magnesium. Magnesium will displace hydrogen in hydrogen chloride because it is more reactive than hydrogen. The displacement reaction is as follow
Mg(s) + HCl(aq) → MgCl(s) + H2(g). The balanced equation with the simplest whole number ratio is as follows
Mg(s) + 2HCl(aq) → MgCl2(s) + H2(g)
