Answer:
5.6L
Explanation:
At STP, the pressure and temperature of an ideal gas is
P = 1 atm
T = 273.15k
Volume =?
Mass = 9.5g
From ideal gas equation,
PV = nRT
P = pressure
V = volume
n = number of moles
R = ideal gas constant =0.082J/mol.K
T = temperature of the ideal gas
Number of moles = mass / molar mass
Molar mass of F2 = 37.99g/mol
Number of moles = mass / molar mass
Number of moles = 9.5 / 37.99
Number of moles = 0.25moles
PV = nRT
V = nRT/ P
V = (0.25 × 0.082 × 273.15) / 1
V = 5.599L = 5.6L
The volume of the gas is 5.6L
They use it because it's standerize and evidence vase
0.300 M IKI represents the
concentration which is in molarity of a potassium iodide solution. This means
that for every liter of solution there are 0.300 moles of potassium iodide. Knowing
that molarity is a ratio of solute to solution.
By using a conversion factor:
100 ml x (1L / 1000 mL) x (0.300
mol Kl / 1 L) x (166.0g / 1 mol Kl) = 4.98 g
Therefore, in the first
conversion by simply converting the unit of volume to liter, Molarity is in L
where the volume is in liters. The next step is converted in moles from volume
by using molarity as a conversion factor which is similar to how density can be
used to convert between volume and mass. After converting to moles it is simply
used as molar mass of Kl which is obtained from periodic table to convert from
mole to grams.
In order to get the grams of IKI
to create a 100 mL solution of 0.600 M IKI, use the same formula as above:
100 ml x (1L / 1000 mL) x (0.600
mol Kl / 1 L) x (166.0g / 1 mol Kl) = 9.96 g
Atomic mass Carbon (C ) = 12.01 a.m.u
12.01 g ---------- 6.02x10²³ atoms
1.50 g ----------- ??
1.50 x ( 6.02x10²³ ) / 12.01 =
7.51x10²² atoms of C
hope this helps!
Assuming the complete question is;
Consider the balanced equation below;
4NH3 + 3O2 = 2N2 +6H2O
What is the mole ratio of NH3 to N2;
From the balanced equation; the mole ratio of NH3 to N2 is 4:2.
The mole ratio is the ratio of moles of one substance to the number of moles of another substance in a balanced equation. In the above equation; 4 moles of ammonia requires 3 moles of oxygen to produce two moles of nitrogen and six moles of water.
