Chemistry questions.. i need help??

Question

If 1.00 mol of CS2 is combined with 1.00 mol of )2,identify the limiting reactant
-How many moles of excess reactant remain?and How many moles of each product are formed???



Can someone help?? please??

Answer 1

1) Set-up the reaction equation:
CS2 + 3 O2 -> CO2 + 2 SO2


2) Find the limiting reagent
You'll need 3 mol of O2 for each mol of CS2
therefore because of so little O2 it will act as a limiting reactant and we will be left with 2/3 mol of CS2

Answer 2

CS2 and what?

first you write the balanced equation
solve for the amount of products through stoich
for both reactants, the lower answer is the limiting reactant
subtract the answer for 1.00 mol and u have ur excess reactant
remain.

Answer 3

What is your second reactant?

CS2 + 3 O2 -> CO2 + 2 SO2

Each mol of CS2 requires 3 mol of O2 so CS2 will be the limiting reactant. Working from that...

(1.0 mol O2)(1.0 mol CS2 / 3mol O2) = 1/3 mol CS2

So 1 mol CS2 - 1/3 mol CS2 would leave 2/3 mol CS2 unused.

For the products use the same equation and their molar ratios.

(1.0 mol O2)(1.0 mol CO2 / 3mol O2) = 1/3 mol CO2

(1.0 mol O2)(2.0 mol SO2 / 3mol O2) = 2/3 mol SO2

Hope this helps.

Answer 4

use a BCA table

CS2 + )2 --> product?
B 1 mol 1 mol -->
C
A

What's the product of CS2 and )2?