0.22g of a hydrocarbon (compound of C & H) on complete combustion with oxygen gave 0.9 g of water and 0.44g carbon dioxide. Show that these are in accordance with law of conservation of mass.
Convert 0.9 g H2O to g H. 0.9 x 2/18 = 0.1
Convert 0.44 g CO2 to C. 0.44/44 x 12 = 0.12
Total = 0.22 which agrees with the starting mass.
To show that the given data is in accordance with the law of conservation of mass, we need to calculate the total mass of the reactants and compare it to the total mass of the products. Let's break down the steps to find the total mass of both sides.
1. First, let's calculate the total mass of the reactants:
The reactants are the hydrocarbon (compound of C and H) and oxygen.
Mass of hydrocarbon = 0.22 g
Mass of oxygen = ?
Since the molecular formula of the hydrocarbon is not provided, we'll have to assume it is a general hydrocarbon represented as CₙHₘ. Therefore, we know that the hydrocarbon contains carbon and hydrogen atoms.
Let's find the mass of carbon and hydrogen in the hydrocarbon:
- Carbon: Since 1 mole of carbon weighs 12 g, we need to count the number of carbon atoms. Let's assume there are n carbon atoms, so the total mass of carbon will be n * 12 g.
- Hydrogen: Since 1 mole of hydrogen weighs 1 g, we need to count the number of hydrogen atoms. Let's assume there are m hydrogen atoms, so the total mass of hydrogen will be m * 1 g.
Therefore, the total mass of the hydrocarbon is equal to the mass of carbon plus the mass of hydrogen:
Mass of hydrocarbon = n * 12 g + m * 1 g
To calculate the mass of oxygen, we can use the concept of the law of conservation of mass, which states that the mass of reactants is equal to the mass of products.
Thus, the total mass of reactants = Mass of hydrocarbon + Mass of oxygen.
2. Now, let's calculate the total mass of the products:
The products are water and carbon dioxide.
Mass of water = 0.9 g
Mass of carbon dioxide = 0.44 g
Therefore, the total mass of the products = Mass of water + Mass of carbon dioxide.
3. Finally, let's compare the total mass of the reactants with the total mass of the products.
According to the law of conservation of mass, these two values should be equal if mass is conserved during the reaction.
Total mass of reactants = Total mass of products
By performing the above calculations, you can check whether the given data is in accordance with the law of conservation of mass.
To show that the given data is in accordance with the law of conservation of mass, we need to calculate the total mass of the products and compare it with the mass of the reactant.
The equation for the complete combustion of the hydrocarbon (CxHy) can be represented as follows:
CxHy + (x + (y/4))O2 → xCO2 + (y/2)H2O
Given that 0.22g of the hydrocarbon produces 0.9g of water and 0.44g of carbon dioxide, we can set up the following equations:
0.9g H2O = (y/2)g H2O
0.44g CO2 = xg CO2
Now, let's solve for x and y:
From the equation, we can see that the ratio of H2O to CO2 is (y/2):(x), which is (0.9g):(0.44g), or 2.045:1.
Hence, y = 2 * 2.045 = 4.09 (approximately 4).
Now, substituting the value of y into the equation for CO2:
0.44g CO2 = xg CO2
0.44g = xg
x ≈ 0.44g
Now, let's calculate the total mass of the products:
Total mass of products = mass of water + mass of carbon dioxide
= 0.9g + 0.44g
= 1.34g
The total mass of the products is approximately 1.34g.
Comparing this with the mass of the reactant, which is 0.22g, we can see that the total mass of the products is greater than the mass of the reactant.
According to the law of conservation of mass, the total mass of the products in a chemical reaction must be equal to the total mass of the reactants. In this case, the total mass of the products exceeds the mass of the reactant, so the law of conservation of mass is not satisfied.
There may be errors in the measurements or experimental procedure. It is possible that some reactants or products were lost during the experiment, leading to a discrepancy in the masses.