Write the symbol for every chemical element that has atomic number less than 75 and atomic mass greater than 173.5 u.
1 answer:
You might be interested in
The empirical formula of the hydrocarbon is if combustion of 8.60 g of a hydrocarbon produced 26.5 g of
and 12.2 g of
.
A chemical formula showing the simplest ratio of elements in a compound rather than the total number of atoms in the molecule is the empirical formula for glucose.
1 mole of carbon dioxide contains a mass of 44 g, out of which 12 g are carbon.
Hence, in this case the mass of carbon in 8.46 g of :
() × 8.46 = 2.3073 g
1 mole of water contains 18 g, out of which 2 g is hydrogen;
Therefore, 2.6 g of water contains;
( × 2.6 = 0.2889 g of hydrogen.
Therefore, with the amount of carbon and hydrogen from the hydrocarbon, we can calculate the empirical formula.
We first calculate the number of moles of each,
Carbon = = 0.1923 moles
Hydrogen = = 0.2889 moles
Then, we calculate the ratio of Carbon to hydrogen by dividing by the smallest number value;
Carbon : Hydrogen
:
1 : 1.5
(1 : 1.5) 2
= 2 : 3
Hence, the empirical formula of the hydrocarbon is .
Learn more about the empirical formula here:
#SPJ1
Answer:
The density of this liquid is 0.320 kg/L
Explanation:
Given:
Volume of the Liquid = 0.820 L
Mass of the liquid = 2.56 kg.
To Find:
The density of the liquid in kg/L
Solution:
Density is the mass occupied by the substance in unit volume. This density is essential determining whether the substance floats or sinks. Greek letter(rho) is used to denote density
The equation of for density is
where m is the mass
v is the volume
On substituting the given values
<u>Answer:</u> The mass of rust that can be removed is 1.597 grams
<u>Explanation:</u>
To calculate the number of moles for given molarity, we use the equation:
.....(1)
Molarity of oxalic acid solution = 0.1255 M
Volume of solution = = 600 mL = 0.600 L (Conversion factor: 1 L = 1000 mL)
Putting values in equation 1, we get:
For the given chemical reaction:
By Stoichiometry of the reaction:
6 moles of oxalic acid reacts with 1 mole of ferric oxide (rust)
So, 0.06 moles of oxalic acid will react with = of ferric oxide (rust)
To calculate the mass of rust for given number of moles, we use the equation:
Molar mass of rust (ferric oxide) = 159.7 g/mol
Moles of rust = 0.01 moles
Putting values in above equation, we get:
Hence, the mass of rust that can be removed is 1.597 grams