Answer:
ΔHrxn = -635.14kJ/mol
Explanation:
We can make algebraic operations of reactions until obtain the desire reaction and, ΔH of the reaction must be operated in the same way to obtain the ΔH of the desire reaction (Hess's law). Using the reactions:
(1)Ca(s) + 2 H+(aq) → Ca2+(aq) + H2(g) ΔH = 1925.9 kJ/mol
(2) 2H2(g) + O2 g) → 2 H2O(l) ΔH = −571.68 kJ/mole
(3) CaO(s) + 2 H+(aq) → Ca2+(aq) + H2O(l) ΔH = 2275.2 kJ/mole
Reaction (1) - (3) produce:
Ca(s) + H2O(l) → H2(g) + CaO(s)
ΔH = 1925.9kJ/mol - 2275.2kJ/mol = -349.3kJ/mol
Now this reaction + 1/2(2):
Ca(s) + ½ O2(g) → CaO(s)
ΔH = -349.3kJ/mol + 1/2 (-571.68kJ/mol)
<h3>ΔHrxn = -635.14kJ/mol</h3>
Carbon is 12 grams per mole
The concentration of a cell is generally 0.15 M (0.9 % NaCl)
As given the solution has concentration = 200mm = 0.02 M
This concentration of solution is less than the concentration of cell
Hence solution is hypotonic (less concentration) and cell will be hypertonic
Answer:
- 0.36 m/s.
Explanation:
- For the reaction: <em>a + 2b → c,</em>
<em>∵ The initial rate of the reaction = - δ[a]/δt = - 1/2 δ[b]/dt = 0.180 m/s.</em>
∴ The initial rate of the reaction = - 1/2 δ[b]/dt = 0.180 m/s.
∴ - 1/2 δ[b]/dt = 0.180 m/s.
<em>∴ δ[b]/dt </em>= (- 2)(0.180 m/s) =<em> - 0.36 m/s.</em>
