A sulphuric plant uses 2500 tonnes of sulphur dioxide each day .What mass of sylph dioxide must be burned to produced quantity of sulphur dioxide
Your post makes no sense at all. In fact it is pointless. Work on it gramatically and repost if you wish to pursue it.
To find the mass of sulfur needed to produce a certain quantity of sulfur dioxide, we need to know the molar ratio between sulfur and sulfur dioxide.
The balanced chemical equation for the combustion of sulfur to produce sulfur dioxide is:
S + O2 → SO2
From the equation, we can see that the molar ratio between sulfur and sulfur dioxide is 1:1, meaning one mole of sulfur reacts to produce one mole of sulfur dioxide.
To determine the mass, we need to convert the given quantity (tonnes) of sulfur dioxide to moles and then back to mass using the molar mass of sulfur.
Given:
Quantity of sulfur dioxide produced = 2500 tonnes
Step 1: Convert tonnes to grams
1 tonne = 1000 kilograms
1 kilogram = 1000 grams
2500 tonnes = 2500 * 1000 * 1000 grams
= 2,500,000,000 grams
Step 2: Convert grams of sulfur dioxide to moles
Molar mass of sulfur dioxide (SO2) = 32.07 g/mol + 2 * 16.00 g/mol
= 64.07 g/mol
Number of moles = (Mass of sulfur dioxide) / (Molar mass of sulfur dioxide)
= 2,500,000,000 g / 64.07 g/mol
≈ 39,036,961 mol
Step 3: Convert moles of sulfur dioxide to moles of sulfur
Since the molar ratio between sulfur and sulfur dioxide is 1:1, the number of moles of sulfur will be the same as the number of moles of sulfur dioxide.
Number of moles of sulfur = 39,036,961 mol
Step 4: Convert moles of sulfur to mass
Molar mass of sulfur (S) = 32.07 g/mol
Mass of sulfur = Number of moles of sulfur * Molar mass of sulfur
= 39,036,961 mol * 32.07 g/mol
≈ 1,251,570,124 g
Therefore, the mass of sulfur that must be burned to produce 2500 tonnes of sulfur dioxide is approximately 1,251,570,124 grams (or 1251.57 tonnes).
To determine the mass of sulfur required to produce a certain quantity of sulfur dioxide, you need to know the molar ratio between the two compounds.
The balanced chemical equation for the combustion of sulfur to produce sulfur dioxide is:
S + O2 -> SO2
According to this equation, one mole of sulfur reacts with one mole of oxygen gas (O2) to produce one mole of sulfur dioxide (SO2). The molar mass of sulfur (S) is approximately 32 g/mol.
To calculate the mass of sulfur required, you can use the following steps:
1. Convert the given quantity (2500 tonnes) to grams:
1 tonne = 1000 kg
1 kg = 1000 g
Therefore, 2500 tonnes = 2500 x 1000 x 1000 g = 2,500,000,000 g
2. Determine the molar mass of sulfur dioxide (SO2):
The molar mass of sulfur (S) is approximately 32 g/mol.
The molar mass of oxygen (O2) is approximately 32 g/mol (16 x 2).
The molar mass of sulfur dioxide (SO2) = 32 g/mol + 32 g/mol = 64 g/mol.
3. Set up a proportion using the molar ratio between sulfur and sulfur dioxide:
Mass of sulfur (unknown) / Molar mass of sulfur = Mass of sulfur dioxide / Molar mass of sulfur dioxide
Mass of sulfur = (Mass of sulfur dioxide / Molar mass of sulfur dioxide) x Molar mass of sulfur.
Plugging in the known values:
Mass of sulfur = (2,500,000,000 g / 64 g/mol) x 32 g/mol = 1,000,000,000 g.
Therefore, to produce the given quantity of sulfur dioxide (2500 tonnes), approximately 1 billion grams (1 million kilograms) of sulfur must be burned.