5C(s) + 2SO2(g) > CS2(l) + 4CO(g)
How many moles of SO2 required to make 17g of CO.
5C(s) + 2SO2(g) > CS2(l) + 4CO(g)
mols CO in 17 g. moles = g/molar mass = 17/30 = 0.567
From the balanced equation you see 2 mols SO2 will produce 4 moles CO; therefore, convert mole CO to mols SO2 as follows: 0.567 mols CO x (2 moles SO2/4 mols CO) = ?
how many moles of CO in 17g?
1/2 that many moles of SO2
So 8.5 moles of SO2
Ok here is what I have so far :
17gCO x 1mol/28.01 g CO x 2molSO2/4 mol CO
I don't have the slightest idea how you came up with 8.5 moles SO2. Your equation is correct; i.e., 17 g CO x (1 mol CO/28.01) x (2 mols SO2/4 mols CO) = ? and it isn't 8.5
To determine the number of moles of SO2 required to produce 17g of CO, we need to use stoichiometry and the balanced chemical equation provided.
The balanced equation is:
5C(s) + 2SO2(g) → CS2(l) + 4CO(g)
Let's first calculate the molar mass of carbon monoxide (CO):
Carbon (C) atomic mass = 12.01 g/mol
Oxygen (O) atomic mass = 16.00 g/mol
Molar mass of CO = Carbon atomic mass + Oxygen atomic mass
= 12.01 g/mol + 16.00 g/mol
= 28.01 g/mol
Now, we can set up a ratio using the coefficients from the balanced equation:
4 moles of CO produced for every 2 moles of SO2
Since we want to find the moles of SO2 required to produce 17g of CO, we can use the following conversion:
17g CO × (1 mol CO / 28.01 g CO) × (2 mol SO2 / 4 mol CO) = moles of SO2
Let's calculate it step by step:
Step 1: Convert 17g of CO to moles of CO.
17g CO × (1 mol CO / 28.01 g CO) = 0.607 mol CO
Step 2: Use the mole ratio from the balanced equation to find moles of SO2.
0.607 mol CO × (2 mol SO2 / 4 mol CO) = 0.3035 mol SO2
Therefore, you would need 0.3035 moles of SO2 to produce 17g of CO.