Answer:
103.7 grams
Explanation:
Al: 1 * 26.98 = 26.98
O: 2 * 16.00 = 32.00
H: 2 * 1.01 = 2.02
26.98 + 32.00 + 2.02 = 61.00
* 
= 103.7 grams of
The answer is the first one!!! have a WONDERFUL day!!
Answer:
Molarity = 0.809 M
mole fraction = 0.047
Explanation:
The complete question is
Calculate the molarity and mole fraction of acetone in a 1.09-molal solution of acetone (CH3COCH3) in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.) Assume that the volumes of acetone and ethanol add.
Solution -
Solution for molarity:
1.09-molal means 1.09 moles of acetone in 1.00 kilogram of ethanol.
1)
Mass of 1.09 mole of acetone
= 1.09 mol x 58.0794 g/mol = 63.306 g
Density of acetone = 0.788 g/cm3
Thus, volume of 1.09 moles of acetone = 63.306 g/0.788 g/cm3 = 80.34 cm3
For ethanol
1000 g divided by 0.789 g/cm3 = 1267.427 cm3
Total volume of the solution = Volume of acetone + Volume of ethanol = 80.34 cm3 + 1267.427 cm3 = 1347.765 cm3 = 1.347 L
a) Molarity:
1.09 mol / 1.347 L = 0.809 M
Mole Fraction
a) moles of ethanol:
1000 g / 46.0684 g/mol = 21.71 mol
b) moles of acetone:
1.09 / (1.09 + 21.71) = 0.047
Answer:
15moles
Explanation:
Given parameters:
Mass of H₂SO₄ = 1469g
Unknown:
Number of moles = ?
Solution:
To solve this problem, let us first find the molar mass of the given compound;
molar mass = 2(1) + 32 + 4(16) = 98g/mol
So;
Number of moles = 
= 
Number of moles = 15moles
Answer:
P₂ = 16.6 atm
Explanation:
Given data:
Initial pressure = 13.0 atm
Initial temperature = 20.0°C (20+273 = 293 K)
Final temperature = 102.0°C (102+273 =375 K)
Final pressure = ?
Solution:
According to Gay-Lussac Law,
The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.
Mathematical relationship:
P₁/T₁ = P₂/T₂
Now we will put the values in formula:
13.0 atm / 293 K = P₂/375 K
P₂ = 13.0 atm × 375 K / 293 K
P₂ = 4875 atm. K /293 K
P₂ = 16.6 atm
