Answer:
Explanation:
10 mL = .01 L .
25 mL = .025 mL .
10 mL of .1 M NaOH will contain .01 x .1 = .001 moles
25 mL of .1M HCl will contain .025 x .1 = .0025 moles
acid will neutralise and after neutralisation moles of acid remaining
= .0025 - .001 = .0015 moles .
Total volume = .01 + .025 = .035 L
concentration of remaining HCl = .0015 / .035
Option D is correct.
= .042857 M
= 42.857 x 10⁻³ M .
pH = - log [42.857 x 10⁻³]
= 3 - log 42.857
= 3 - 1.632
= 1.368 .
Answer:
Explanation:
equilibrium constant
Kc = [ C ]² / [ A ] [ B ]
= .5² / .2 x 3
= .4167
Let moles of A to be added be n
concentration of A unreacted becomes .2 + n M
increase of product C by .2 M will require use of A and B be .1 M
So unreacted A = .2 + n - .1 = n + .1
Kc = [ C ]² / [ A ] [ B ]
.4167 = .7² / ( n + .1 ) ( 3 - .1 )
n + .1 = .4
n = . 3 moles .
So .3 moles of A to be added .
Osazones<span> are a class of carbohydrate derivatives found in organic chemistry formed when sugars are reacted with excess of phenylhydrazine. The famous German chemist Emil Fischer developed and used the reaction to identify sugars whose stereochemistry differed by only one chiral carbon</span>
Answer:
D
Explanation:
Diabetes is caused when the pancreas has trouble producing insulin, a hormone that lowers blood sugar levels. Since the endocrine system deals with hormones, diabetes is an endocrine system disease.
Answer:
ΔGreaction < 0
ΔSuniverse > 0
ΔHreaction < 0
Explanation:
A spontaneous process is one which can proceed without additional input of energy releasing free energy in the process and then moves to a lower more stable thermodynamical state.
For an isolated system, a spontaneous process proceeds with an increase in entropy.
The conditions for a spontaneous process at constant temperature and pressure, can be determined using the change in Gibbs free energy, which is given by: ∆G = ∆H - T∆S
Where ∆G is change in free energy; ∆H is change in enthalpy or Heat content; ∆S is change in entropy, T is temperature.
For a process to be spontaneous, the following conditions are necessary:
1. ∆G < 0; must be negative
2. ∆S > 0; there must be an increase in entropy
3. ∆H < 0; enthalpy change must be negative such that heat is lost to the surroundings
The above conditions ensures that ∆G is negative and the process is spontaneous.
