calculate the volume of O2 at STP for the complete combustion of two moles of carbon disulphide which produces CO2 and SO2.

i think 134.4 dm3.

Please can u give the solution to it :/

2CS2 + 6O2 -> 2CO2 + 4SO2

So, now you know that you will need 6 moles of O2. What is the volume of 6 moles of any gas at STP?

That's correct.

Numerical s of stoichiometry volume to mass realtion ship

To calculate the volume of O2 at STP for the complete combustion of carbon disulphide (CS2), we need to use the balanced chemical equation for the reaction and the ideal gas law.

The balanced equation for the combustion of CS2 is:
CS2 + 3O2 → CO2 + 2SO2

From the equation, we can see that 1 mole of CS2 reacts with 3 moles of O2 to produce 1 mole of CO2 and 2 moles of SO2.

Given that we have 2 moles of CS2, we can calculate the moles of O2 required based on the stoichiometry of the balanced equation.

2 moles CS2 × (3 moles O2 / 1 mole CS2) = 6 moles O2

Now, we can use the ideal gas law to calculate the volume of O2 at STP.

The ideal gas law equation is:
PV = nRT

Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L•atm/(mol•K))
T = temperature (in Kelvin)

At STP (Standard Temperature and Pressure), the temperature is 273.15 K and the pressure is 1 atm.

n = 6 moles
R = 0.0821 L•atm/(mol•K)
T = 273.15 K
P = 1 atm

Plugging in these values into the ideal gas law equation, we can solve for the volume V:

V = (nRT) / P
= (6 moles)(0.0821 L•atm/(mol•K))(273.15 K) / (1 atm)
≈ 132.2 liters

Therefore, the volume of O2 at STP for the complete combustion of two moles of CS2 is approximately 132.2 liters.