Iron reacts with oxygen to produce iron(III) oxide: (a) 4 Fe + 3 O( → 2 Fe(O+ (a) Write the mole ratio between Fe and O2 in the balanced chemical equation: (b) How many moles of Fe2O3 are produced from 1.4 moles of Fe? Show your work.

Given the unbalanced chemical equation, CH3OH(I) + O2(g) CO2(g) + H20(g), what is the mole ratio between CH3OH and CO2 (CH;OH:CO2)? O 2:1 O 1:1 O 3:2 O 1:2

This question has two parts and requires two answers. Consider the reaction 4 Fe + 3 02→ 2 Fe203 a) What is the theoretical yield, in grams, of iron(III) oxide if 20.0 g of iron are mixed with 10.5 grams of oxygen gas? b) What is the limiting reactant?

This question has multiple parts: The following equation represents the formation of water from hydrogen gas and oxygen gas: H 2 (g)+ O 2 (g) H 2 O(l) (a) Balance the equation . (b) Refer to your balanced equation. If 5.0 g of hydrogen gas is reacted with 15.0 g of oxygen gas , what is the limiting reagent ? How many grams of water are produced theoretically , If only 5.0 g of water is actually produced , what is the percent yield?

What is the mass in grams of CO, that can be produced from the combustion of 2.76 moles of butane according to this equation: 2 C,H10(g) + 13 02(g) → 8 CO2(g) + 10 H,0(g)

Can you please solve all five questions for me? Chemistry

For the following reaction, give the balanced equation for the reaction. PBr3 (1) + 3H₂O(1) → H3PO3(aq) + 3HBr(g) mol PBr3 mol H₂O mol H3PO3 mol HBr

Metal hydrides react with water to form hydrogen gas and metal hydroxide. For example, SrH2(s) + 2H2O(l) → Sr(OH)2(s) + 2H2(g) You wish to calculate the mass of hydrogen gas that can be prepared from 2.81 g of SrH2 and 2.34 g of H2O. (a) How many moles of H2 can be produced from the given mass of SrH2?(b) How many moles of H2 can be produced from the given mass of H2O? (c) Which is the limiting reactant? (d) How many grams of H2 can be produced?

An experiment that led to the formation of the new field of organic chemistry involved the synthesis of urea, CN2H4O, by the controlled reaction of ammonia and carbon dioxide:2 NH3 (g) + CO2 (g) → CN2H4O (s) + H2O (l)What is the theoretical yield of urea when 100. g of ammonia is reacted with 100.g of carbon dioxide?

The steel-making process described in the Transition Metal section of the Elements Handbook shows the equation for the formation of iron carbide. Use this equation (given below) to answer the following questions. 3 Fe + C  Fe3C (a) If 3.79 ✕ 103 kg of iron is used in a steel-making process, what is the minimum mass of carbon needed to react with all of the iron? kg(b) What is the theoretical mass of iron carbide that is formed? kg