Answer:
Explanation:
In KCl, the two elements that combine to create KCl are potassium (K) and chlorine (Cl).
Potassium, as a Group 1 element, possesses one valence electron in its outermost shell which it readily donates during bonding. Every element aims to achieve a stable electron configuration, typically with 2 or 8 electrons in its outer shell. Potassium is characterized by its lower electronegativity and higher ionization energy, making it more likely to donate its electron than to accept one. On the other hand, chlorine belongs to Group 17 and has 7 electrons in its outer shell, requiring just one additional electron to complete its octet. Chlorine’s higher electronegativity and lower ionization energy facilitate its tendency to accept an electron rather than donate it.
The bond between potassium and chlorine that results in KCl is termed an electrovalent bond.
Reaction equation:
K + Cl → KCl
1) The chemical equation is
Cu + 2AgNO3 ---> Cu (NO3)2 + 2Ag
2) Molar ratios are as follows:
1 mol Cu: 2 moles AgNO3: 1 mol Cu (NO3)2: 2 mol Ag
3) Converting 12.83 * 10^23 atoms of Cu to moles gives:
12.83 * 10^23 atoms / (6.02 * 10^23 atoms / mol) = 2.131 mol Cu
4) Using the ratios:
2.131 mol Cu * 2 mol Ag / 1 mol Cu = 4.262 mol Ag
5) To convert 4.262 mol of silver to grams, use the atomic weight of silver:
mass = moles × atomic mass = 4.262 mol * 107.9 g / mol = 459.9 grams
Answer: 459.9 g
Answer:
The correct option is C. 21900.3. I calculated 21945 J, which makes option C closely aligned with my result.
Explanation:
Data
mass = 150 g
initial temperature T1 = 10°C
final temperature T2 = 45°C
Cw = 4.18 J/g°C
Formula
Q = mCΔT = mC(T2 - T1)
Substitution
Q = (150)(4.18)(45 - 10)
Simplification
Q = (150)(4.18)(35)
Result
Q = 21945 J
The correct equation is (C) H3O+(aq) + C2H3O2−(aq) -> HC2H3O2(aq) + H2O(l). A buffer system is composed of a weak acid and its corresponding salt, effectively stabilizing the pH levels within a solution. The buffer works by adjusting the concentrations of the conjugate acid and base, maintaining the pH constant.
The specific heat of titanium metal is 0.524 J/g°C. Given that Q = 1.68 kJ, which equates to 1680 Joules, with a mass of 126 grams and initial and final temperatures of 20°C and 45.4°C respectively, the specific heat is computed using the formula Q = (mass)(ΔT)(Cp), where ΔT = T₂ - T₁ = 25.4°C. Plugging in the numbers leads us to Cp = 0.524 J/g°C.
