Based on the data given, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu
<h3>How can molar mass of a gas be obtained from density, temperature and pressure?</h3>
The molar mass of a gas can be obtained from density, temperature and pressure using the formula below:
- molar mass = density × molar gas constant × temperature/pressure
Molar gas constant, R = R = 0.082 L.atm/mol/K.
Temperature = 150 °C = 423 K
Pressure = 785 torr = 1.033 atm
density = 4.93 g/L
molar mass of gas = 4.93 × 0.082 × 423/1.033
molar mass of gas = 165.5 g/mol
Then, molecular weight of the gas = 165.5 amu
Therefore, the molar mass of the gas is 165.5 g/mol while the molecular weight of the gas is 165.5 amu
Learn more about molar mass of a gas at: brainly.com/question/26215522
Answer:
c MgO
Explanation:
product is located after the reaction arrow
Answer:A) It was developed from past observations- true
It is subject to experimentation and revision.- false
It explains why mass is conserved- false
It predicts future observations-true
Explanation:
Before a hypothesis is proclaimed to be a law in science, numerous observation must have confirmed its validity and rigorous experimentation under carefully controlled conditions usually precedes the acceptance of a hypothesis as a law. The law of conservation of mass was developed from numerous past observation that proved its validity.
3.
∆E = ∆m x c ² ∆m = E / c ² ∆m = 3,83•10^-12 / 3•10^8 ² ∆m = 4,256•10^-29 kg
Taking this class as well
4X + 3O₂ = 2X₂O₃
n(X₂O₃)=0.02225 mol
m(X)=4.000 g
x - the molar mass of metal
m(X)/4x=n(X₂O₃)/2
x=m(X)/{2n(X₂O₃)}
x=4.000/{2*0.02225)=89.89 g/mol
X=Y (yttrium)
