Nice written.
Is it written by you yourself or you have copied it from somewhere?
<span>There are a number of ways
to express concentration of a solution. This includes molarity. Molarity is
expressed as the number of moles of solute per volume of the solution.
Calculations are as follows:
Molarity of NO3 ion = 32.0 g Mg(NO3)2 ( 1 mol / 148.3 g ) ( 2 mol NO3 / 1 mol Mg(NO3)2) / .425 L
MOlarity of NO3 ion = 1.02 M </span><span>
</span>
Answer:
The required volume is 1.12 L.
Explanation:
Given,
Mass of O2 gas= 1.60 grams
We know,
Number of moles = Mass/Molecular mass
= 1.60/32 [Molecular mass of O2 gas is 32 gram]
= 0.05
Again,
We know that at STP,
Number of moles = Volume in L / 22.4 L
or, Volume = Number of moles X 22.4
or, Volume = 0.05 X 22.4
or, Volume = 1.12
∴The required volume is 1.12 L.
Answer:
16.89 atm.
Explanation:
Step 1:
Data obtained from the question
Number of mole (n) = 2.3 mol
Temperature (T) = 40°C = 40°C + 273 = 313K
Volume (V) = 3.5L
Pressure (P) =..?
Gas constant (R) =0.0821 atm.L/Kmol
The pressure exerted by the gas can be obtained by using the ideal gas equation as shown below:
PV = nRT
Divide both side by V
P = nRT /V
P = 2.3 x 0.0821 x 313 / 3.5
P = 16.89 atm.
Therefore, the pressure exerted by the gas is 16.89 atm.
Answer:
1.02 × 10⁻³ g
Explanation:
Step 1: Given data
Number of moles of titanium (IV) oxide in 1 jelly bean (n): 1.28 × 10⁻⁵ moles
Step 2: Calculate the mass (in grams) corresponding to 1.28 × 10⁻⁵ moles of TiO₂
To convert moles to mass, we need a conversion factor. In this case, it is the molar mass of TiO₂: 79.87 g/mol.
1.28 × 10⁻⁵ mol TiO₂ × 79.87 g TiO₂/1 mol TiO₂ = 1.02 × 10⁻³ g TiO₂
