Answer:
1.8 moles of O₂
Explanation:
The balance chemical equation for said double replacement (photosynthesis) reaction is as follow;
6 CO₂ + 6 H₂O → C₆H₁₂O₆ + 6 O₂
According to balance chemical equation,
6 moles of O₂ are produced by = 6 moles of CO₂
So,
1.8 moles of O₂ will be produced by = X moles of O₂
Solving for X,
X = 1.8 mol × 6 mol / 6 mol
X = 1.8 moles of O₂
Stoichiometric problems in which moles are given and moles or other reactant or product asked are the simplest problems. One should only write the balanced chemical equation and perform above method to find the required moles.
It might be more suitable because some data cannot use a graph to show data because there is too much data.
Overall, an atom is neutral charged. The Bohr model was for years accepted as the final authority because it agrees so well with experiment and observation. In this model an atom consists of a nucleus containing protons and neutrons. The neutrons are zero charge so we can forget them in looking for charges. For each proton (1 positive charge) there is always 1 electron (1 negative charge) in orbit around the nucleus. thus an atom has a equal number of electrons and protons and their net charge is zero.
We can do things to temporarily up set this natural balance (we call this electricity) but the atoms will eventually return to their naturally balanced state
Answer: Ferrous metals, non ferrous metals and alloys.
Explanation:
Answer:
The equilibrium constant Kc = [Fe]²*[H2O]³ / [Fe2O3][H2]³
Explanation:
Step 1: Data given
For the reaction aA + bB ⇆ cC + dD
the equilibrium constant Kc = [C]^c * [D]^d/[B]^b*[A]^a
Step 2: The balanced equation
Fe2O3(s) + 3H2(g) --> 2Fe(s) + 3H2O(g)
Step 3: Calculate the equilibrium constant Kc
Kc = [C]^c * [D]^d/[B]^b*[A]^a
⇒with [C] = [Fe]
⇒ with c = 2
⇒with [D] = [H2O]
⇒with d = 3
⇒with [A] = [Fe2O3]
⇒with a = 1
⇒with [B] = [H2]
⇒with b = 3
Kc = [C]^c * [D]^d/[B]^b*[A]^a
Kc = [Fe]²*[H2O]³ / [Fe2O3][H2]³
The equilibrium constant Kc = [Fe]²*[H2O]³ / [Fe2O3][H2]³
