What mass of co is needed to react completely with 55.0 g of fe2o3 in the reaction: fe2o3(s) + co(g) → fe(s) + co2(g)? 4.82 g co 9.64 g co 14.5 g co 28.9 g co

- 28.9 grams of CO are needed to react with 55.0 grams of Iron(II)oxide.

Solution:- The balanced equation for the given reaction is:

From this equation, 1 mol of Iron(II)oxide reacts with 2 moles of carbon monoxide. First of all we convert given grams of Iron(II)oxide to moles and multiply by the mol ratio to get the moles of CO. Further the moles of CO are multiplied by it's molar mass to find out it's grams.

Molar mass of is 159.69 gram per mol and the molar mass of CO is 28 gram per mol. The calculations are shown below:

= 28.9 g CO

So, 28.9 grams of CO are needed to react completely with 55.0 grams of Iron(II)oxide.

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.