Used the following equation to answer the question below : 5C(s)+2SO2(g)=CS2(I)+4CO(q)
A-) how many moles of carbon needed to produce 13g of CS2.
B-) how many grams of SO2 are necessary to react with 3.45g of carbon.
C-) how many liters of CO (at STP) re produced from 2.45 mole of SO2?
how many moles in 13g of CS2?
The equation tells you that it takes 5 times that many moles of C.
same for SO2. Figure the moles of C, then take 2/5 that many of SO2. Then go back to grams.
Again, figure the moles, and recall that one mole of a gas occupies 22.4L at STP.
To answer these questions, we need to use stoichiometry, which is a method of relating the amounts of reactants and products in a chemical equation. In this case, we will use the balanced chemical equation:
5C(s) + 2SO2(g) = CS2(l) + 4CO(g)
A) To find the number of moles of carbon needed to produce 13g of CS2, we can use the molar ratio between carbon and CS2 from the balanced equation. The ratio is 5 moles of carbon to 1 mole of CS2.
Molar mass of CS2: C = 12.01 g/mol, S = 32.07 g/mol
Total molar mass of CS2: 12.01 g/mol * 1 + 32.07 g/mol * 2 = 76.15 g/mol
Number of moles of CS2 = mass / molar mass
Number of moles of CS2 = 13g / 76.15 g/mol = 0.1704 mol
According to the molar ratio, the number of moles of carbon needed is:
Number of moles of carbon = 5 * 0.1704 mol = 0.8520 mol
So, 0.8520 moles of carbon are needed to produce 13g of CS2.
B) To find the grams of SO2 necessary to react with 3.45g of carbon, we use the molar mass and the molar ratio between carbon and SO2. The ratio is 5 moles of carbon to 2 moles of SO2.
Number of moles of carbon = mass / molar mass
Number of moles of carbon = 3.45g / 12.01 g/mol = 0.2864 mol
According to the molar ratio, the number of moles of SO2 needed is:
Number of moles of SO2 = 2/5 * 0.2864 mol = 0.1146 mol
Now we can calculate the grams of SO2 needed:
grams of SO2 = number of moles * molar mass
grams of SO2 = 0.1146 mol * 64.07 g/mol = 7.34g
Therefore, 7.34 grams of SO2 are necessary to react with 3.45 grams of carbon.
C) To find the number of liters of CO gas produced from 2.45 moles of SO2 at STP, we need to use the ideal gas law and the molar ratio between SO2 and CO. The ratio is 2 moles of SO2 to 4 moles of CO.
Number of moles of SO2 = 2.45 mol
According to the molar ratio, the number of moles of CO produced is:
Number of moles of CO = 4/2 * 2.45 mol = 4.90 mol
At STP (Standard Temperature and Pressure), 1 mole of an ideal gas occupies 22.4 liters. So,
Number of liters of CO = 4.90 mol * 22.4 L/mol = 109.36 L
Therefore, 109.36 liters of CO gas are produced from 2.45 moles of SO2 at STP.