Question

The compound P4S3 is used in matches and reacts with oxygen through the chemical reaction shown below.

What mass of SO2 is produced from the combustion of 0.200 g P4S3?
P4S3 (s) + ------- O2 (g) ===> ------------ P4O10(s) + ----- SO2 (g)

Answer 1

`m_(SO_2)=0.175gSO_2`

Step-by-step explanation:

Hello,

In this case, since the first step is to write the properly balanced chemical reaction:

`P_4S_3 (s) + 8O_2 (g)\rightarrow P_4O_(10)(s) + 3SO_2 (g)`

We can see that given the 0.200 g of P4S3 (molar mass 220 g/mol) the mole ratio between it and SO2 (molar mass 64 g/mol) is 1:3, therefore, the produced mass of SO2 turns out:

`m_(SO_2)=0.200gP_4S_3*(1molP_4S_3)/(220gP_4S_3) *(3molSO_2)/(1molP_4S_3) *(64gSO_2)/(1molSO_2) \\\\m_(SO_2)=0.175gSO_2`

Best regards.