Consider the following chemical reaction: 2CH3OH(l) + 3O2(g) -------> 2CO2(g) + 4H2O(l)  Calculate the number of moles of CO2 produced when 1.154E1 mL of methanol CH3OH(l) reacted completely with O2 (g). The density of methanol is 0.79 g/mL

In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide. CO2 + 2 LiOH = Li2CO3 + H2O If 20 moles of CO2 is exhaled, the average amount exhaleed by a person each day, how much (in grams) Li2CO3 is produced?

The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO,(G) + 0,(g) 2M1O,(G) + 2C0, (g) In the second step, manganese(IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO, (s) + 4Al(s) 3 Mn(s) + 2 Al,O3 (s) Suppose the yield of the first step is 95.% and the yield of the second step is 84.%. Calculate the mass of manganese(II) carbonate required to make 10.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. olo

Consider the reaction 4Fe(s) +302(g) --> 2FE203(s) If you started with and consumed 4 moles of O2, how many moles of Fe2O3 would you produce?

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Consider the reaction 3X + 2Y → 5C + 4D How many moles of C can be synthesized from 37.0 moles of Y and excess X?

In the reaction below, 20.0g of Al2(SO4)3 was mixed with 20.0g of NaOH.       The chemical equation given: Al2(SO4)3+ NaOH= Al(OH)3+Na2SO4 Part 1:) Balance the reaction Part 2:) Determine the limiting reactant and calculate the maximum mass of Al(OH)3 that can be produced Part 3:) state the excess reactant and calculate the mass left over of this reactant.

A mixture of 20.6 gof P and 78.0 g of Cl2 reacts completely to form PCl3 and PCl5 as the only products.  Find the mass of PCl3 that forms. So for the balance chemical equation i got 2P + 4Cl2 ----> PCl3 +PCl5 and for the answer i got 37.76g of PCl3 but it is wrong.

Determine the mass in grams of CO₂ that are produced by the complete reaction of 0.05090 moles of C₇H₈ (toluene) according to the following combustion reaction: C₇H₈(l)+ 9 O₂(g) → 7 CO₂(g) + 4 H₂O(g)

4E  how do you solve for mass when it includes percentage