ard free energy G° by 18 kJ/mole, with A* having the higher G°.
Use the table below to find how many more molecules will be in state A* compared with state A at equilibrium.
If an enzyme lowered the activation energy of the reaction by 11.7 kJ/mole, how would the ratio of A to A* change?
Table: RELATIONSHIP BETWEEN THE STANDARD FREE- ENERGY CHANGE, ∆G°, AND THE EQUILIBRIUM CONSTANT
Hint: ∆G° represents the free-energy difference under standard conditions (where all components are present at a concentration of 1 mole/litter). From this table, we see that if there is a favourable free-energy change of –17.8 kJ/mole for the transition Y→ X, there will be 1000 times more molecules of X than of Y at equilibrium (K = 1000).
nds are a girl’s best friend. So in other words, diamonds and sugar make everything better. What is the common denominator? Carbon! Carbon, under pressure for a long time, makes diamonds. Sugar is a carbon chain. So carbon is good!
How many spoonfuls of sugar C12H22O11 will it take, under pressure for a very very long time, to create another Hope Diamond (45.52 carats)?
How many moles of sugar is this?
How many molecules of sugar is this?
How many atoms of carbon is this?
How many atoms of carbon make the medicine go down?
A carat is equivalent to exactly 200 mg
Sugar has a density of 1.59 g/cm3
A diamond is made entirely of carbon
estimated he consumed 12, 000 kcal/day.
Given that the formation of one ATP molecule from ADP and inorganic phosphate, requires 7.3 kcal/mole and that aerobic respiration is only 34% efficient, how many ATP molecules did Michael Phelps produce each day?
Reminder: There are 6.022 x 10^23 molecules/mole.
bundance of isotope I is (1.94x10^1)%, what would be the calculated atomic mass (in amu)?
2) A hypothetical element exists as two isotopes: I = 78.00 amu and II = 84.00 amu. If the atomic mass of this element is found to be 80.33 amu, which isotope must be more abundant?
3) If the hypothetical polyatomic ion ThOM2- is called "thomite", what would be the formula and name of the acid formed by this ion?
4) How many atoms of hydrogen are there in a sample of (4.00x10^2) grams of NH3(g)?
5) How many O (oxygen) atoms are there in (6.40x10^2) grams of H3PO4?
6) How many moles of fluorine atoms are there in (5.80x10^2) grams of SF4?
7) When 3.50 g of titanium (Ti) reacts with oxygen, the resulting oxide compound weighs 5.84 g. What is the empirical formula of this oxide?
8) How many moles of molecules are there in (6.70x10^2) grams of CH4?
9) A chemical is found to be 80.0% C and the rest is H. If the molar mass of this chemical is known to be 90.2 g/mol, what is the molecular formula?