Answer:
0.908 L.
Explanation:
- Firstly, we should calculate the number of moles of 1.60 g argon.
- n of Ar = mass / molar mass of Ar = (1.60 g) / (39.948 g/mol) = 0.04 mol.
- |t is established and known that the molar volume of a gas at STP (Standard Temperature and Pressure) is equal to 22.4 L for 1 mole of any ideal gas at a temperature of 273.15 K and a pressure of 1.00 atm.
<u><em>using cross multiplication:</em></u>
1.0 mole of Ar gas will occupy → 22.7 L
0.04 mole of Ar gas will occupy → ??? L
∴ The volume occupied by Ar = (0.04 mole) (22.7 L) / (1.0 mole) = 0.908 L.
The best and most correct answer among the choices provided by the question is the third choice. A theory stating <span>particles of all matter are in constant random motion would be the kinetic theory. I </span><span>hope my answer has come to your help. God bless and have a nice day ahead!</span>
Answer:
311.25k
Explanation:
The question assumes heat is not lost to the surroundings, therefore
heat emitted from hotter sample ( 
)= heat absorbed by the less hotter sample( 
)
The relationship between heat (q), mass (m) and temperature (t) is 
where c is specific heat capacity, 
temperature change.
= 
equating both heat emitted and absorb
where the values with subset 1 are the values of the hotter sample of water and the values with subset 2 are the values of the less hot sample of water.
C will cancel out since both are water and they have the same specific heat capacity.
so we have
where m1 = 50g, t 1initial = 330, m2 = 30g, t2 initial = 280,t final (final temperature of the mixture) = ?
-50 * (
- 330) = 30 * ( - 280)
-50 + 16500 = 30 - 8400
80 = 16500+8400
80 = 24900
= 24900/80 = 311.25k
Answer:
The general formula for a straight chain alkane is CnH(2n+...so correct option is C and D
