Answer:
The specific heat of zinc is 0.361 J/g°C
Explanation:
<u>Step 1:</u> Data given
44.0 J needed
Mass of solid zinc = 10.6 grams
Initial temperature = 24.9 °C
Final temperature = 36.4 °C
<u>Step 2</u>: Calculate the specific heat of zinc
Q = m*c*ΔT
⇒ with Q = heat (in Joule) = 44.0 J
⇒ with m = the mass of the solid zinc = 10.6 grams
⇒ with c = the specific heat of the zinc = TO BE DETERMINED
⇒ with ΔT = The change in temperature = T2-T1 = 36.4 °C - 24.9 °C = 11.5 °C
44.0 J = 10.6 grams * c * 11.5°C
c = 44.0 J / (10.6g * 11.5 °C)
c = 0.361 J/g°C
The specific heat of zinc is 0.361 J/g°C
Answer: When an acidic solution is diluted with water the concentration of H + ions decreases and the pH of the solution increases towards 7.
Explanation:
FeC13=1 atom of Fe, 3 atoms of CI
Answer:
The net ionic equation is
H₃O⁺+NH₃ ↔ NH₄⁺+H₂O
Explanation:
To write the net ionic equation, we are required to dissociate the into ions all strong acids and strong bases
Hence, nitric acid which is a strong acid is dissociated as follows
HNO₃+H₂O → H₃O⁺ + NO₃⁻
in the above equation, the nitrate ion NO₃⁻, is a spectator ion because it is only present and does not partake in the chemical reaction so it is left out of the net ionic equation equation
Also the it is required to keep together weak bases in the solution therefore for NH₃ which is a weak base we have
NH₃ + H₃O⁺ → NH₄⁺ + H₂O
Hence, the net ionic equation becomes
H₃O⁺ (aq) + NH₃ ↔ NH₄⁺(aq) + H₂O (l)
The color emitted be larger atoms is lower in energy then the light emitted by smaller atoms
