How many moles of carbon monoxide form at the same time that 0.337 mol CS2 forms?
When? How? Where? what reaction?
how many grams of precipitate are produced when 0.300 M K2CrO4(aq) (50.0mL) are added to excess BaCl2(aq)?
To determine the number of moles of carbon monoxide (CO) that form when 0.337 moles of carbon disulfide (CS2) form, we need to use the balanced chemical equation for the reaction.
The balanced chemical equation is:
CS2 + 3O2 -> CO2 + 2SO2
According to the equation, 1 mole of CS2 reacts with 3 moles of O2 to produce 1 mole of CO2 and 2 moles of SO2. Therefore, the ratio of moles of CS2 to moles of CO2 is 1:1.
Given that 0.337 moles of CS2 form, we can conclude that the same amount of moles of CO2 will form.
Therefore, 0.337 moles of CO will also form at the same time.
To determine the number of moles of carbon monoxide (CO) formed when 0.337 moles of CS2 are formed, we need to use the balanced chemical equation for the reaction between CS2 and CO.
The balanced chemical equation is as follows:
CS2 + 3O2 -> CO2 + 2SO2
According to the balanced equation, one mole of CS2 reacts to form one mole of CO2. This means that the number of moles of carbon monoxide formed will be equal to the number of moles of CS2 formed.
Therefore, if 0.337 moles of CS2 form, 0.337 moles of carbon monoxide will also form at the same time.