Given the unbalanced equation CO2 + H2→ CH4 + H20 (a) How many moles of water can be produced from 16 moles of carbon dioxide? (b) How many moles of CH4 will be produced along with 12 moles of water?

Write a balanced chemical equation based on the following description: solid tetraphosphorus (P₄) reacts with oxygen gas to produce solid tetraphosphorus decoxide. P4(s)+O2(g)_

if 5.7kg of CO2 are produced during a combustion reaction, how many molecules of Co2 would be produced?

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?

Write a balanced chemical equation based on the following description: nitrogen gas reacts with oxygen gas to produce nitrogen monoxide gas N2(g)+O2(g)_

2Hx + Oze → 2H;Om For the combination reaction above between oxygen gas and hydrogen gas to produce water, how many moles of oxygen gas are required to produce 15.0 mol of water? 7.

Aspirin can be made in the laboratory by reacting acetic anhydride (C4H6O3C4H6O3) with salicylic acid (C7H6O3C7H6O3) to form aspirin (C9H8O4C9H8O4) and acetic acid (C2H4O2C2H4O2). The balanced equation isC4H6O3+C7H6O3→C9H8O4+C2H4O2C4H6O3+C7H6O3→C9H8O4+C2H4O2In a laboratory synthesis, a student begins with 3.10 mLmL of acetic anhydride (density=1.08gml−1density=1.08gml−1) and 1.23 gg of salicylic acid. Once the reaction is complete, the student collects 1.22 gg of aspirin.    Determine the percent yield of aspirin for the reaction. Express your answer using three significant figures.

Balance the following chemical equation (if necessary) for the combustion reaction of propane C3H8(g)+O2(g)_CO2(g)+H2O(g)

If sodium peroxide is added to water, elemental oxygen gas is generated, consider this unbalanced equation: Naz O2 (s) + H2 O(1) → NAOH(aq) + 02(9) Suppose 5.80 g of sodium peroxide is added to a large excess of water. What mass of oxygen gas will be produced? Mass =

If 6.5 kg of CO₂ are produced during a combustion reaction, how many molecules of CO₂ would be produced?