The mass of nitrogen collected is mathematically given as
M-N2=0.025gram
<h3>What is the mass of nitrogen collected?</h3>
Question Parameters:
A sample weighing 2.000g
the liberated NH3 is caught in 50ml pipeful of H2SO4 (1.000ml = 0.01860g Na2O).
T=26.3c=299.3K
Pressure=745mmHg=745torr
Pressure of N2=745-25.2=719.8torr
Generally, the equation for the ideal gas is mathematically given as
PV=nRT
Therefore
719.8/760=45.6/1000=n*0.0821*299.3
n=0.00176*14
In conclusion, the Mass of N2
M-N2=0.00176*14
M-N2=0.025gram
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brainly.com/question/4931057
Spring tides occur during the fullmoon and the new moon
Answer:
Immiscible
Explanation:
Immiscible is the term that is used to refer to a mixture of liquids which can separate into distinct layers when left undisturbed. This usually comes to play when a polar solvent such as water is mixed with a non polar solvent such as kerosene.
These two liquids can be made to separate from each other using the method of separatory funnel
Answer: A composite volcano is the most common type of volcano. They have non-explosion and explosion eruptions. There crater is big, or small. They are also called Stratovolcanoes.
Explanation:
Answer:
Mass = 1.84 g
Explanation:
Given data:
Total pressure = 3.44 atm
Volume of flask = 9.62 L
Temperature = 63°C = 63+273.15K = 336.15 K
Mass of CO₂ = 12.5 g
Mass of hydrogen = ?
Solution:
Number of moles of CO₂:
Number of moles = mass/molar mass
Number of moles = 12.5 g/ 44 g/mol
Number of moles = 0.28 mol
Pressure of CO₂:
PV = nRT
R = general gas constant = 0.0821 atm.L/mol.K
P = 0.28 mol × 0.0821 atm.L/mol.K × 336.15 K / 9.62 L
P = 7.73 atm.L/ 9.62 L
P = 0.8 atm
Total pressure = Partial pressure of CO₂ + Partial pressure of H₂
3.44 atm = 0.8 atm + P(H₂)
P(H₂) = 3.44 atm - 0.8 atm
P(H₂) = 2.64 atm
Number of moles of hydrogen:
PV = nRT
2.64 atm × 9.62 L = n × 0.0821 atm.L/mol.K × 336.15 K
25.39 atm.L = n × 27.59atm.L/mol
n = 25.39 atm.L / 27.59atm.L/mol
n = 0.92 mol
Mass of hydrogen:
Mass = number of moles × molar mass
Mass = 0.92 mol × 2 g/mol
Mass = 1.84 g
