Answer:
K⁺ (aq) + F⁻ (aq) + H⁺ (aq) + Cl⁻ (aq) → KCl (aq) + H⁺ (aq) + F⁻ (aq)
Explanation:
KF (aq) + HCl (aq) → KCl (aq) + HF (aq)
KF (aq) → K⁺ (aq) + F⁻ (aq)
HCl (aq) → H⁺ (aq) + Cl⁻ (aq)
KCl (aq) → K⁺ (aq) + Cl⁻ (aq)
HF (aq) → H⁺ (aq) + F⁻ (aq)
Answer:
D = Mass = 42.6 g
Explanation:
Given data:
Mass of phosphorus react = 33 g
Mass of oxygen needed = ?
Solution:
Chemical equation:
4P + 5O₂ → 2P₂O₅
Number of moles of phosphorus:
Number of moles = mass/molar mass
Number of moles = 33 g/ 30.97 g/mol
Number of moles = 1.065 mol
now we will compare the moles of phosphorus and oxygen.
P : O₂
4 : 5
1.065 : 5/4×1.065 = 1.33mol
Mass of oxygen needed:
Mass = number of moles × molar mass
Mass = 1.33 mol × 32 g/mol
Mass = 42.6 g
Thus, 43.6 g of oxygen needed to react with 33 g of phosphorus.
C. It show how many moles are used of each substance.
Answer:
Okay, I think I may actually have an answer for you. I would go with C, "The number of particles able to undergo a chemical reaction is less than the number that is not able to."
Explanation:
I just took a quiz with a similar question, and B is the only gas particle that is able to react. This cancels out all the other answers, as A and B are obviously incorrect based on that information, and it rules out D because T1 is the only sample with a particle able to react. I hope this helps!
