For the following systems at equilibrium

1. CaCO3(s) <-> CaO(s) +CO2 (g) Delta H = +178 kJ/mol
2. PCl3(g) + Cl2(g) <-> PCl5 (g) Delta H= -88 kJ/mol

classify these changes by their effectt

(a) system 1 increase temp:
(b) system1 decrease temp:
(c) system 2 increase temp:
(d) system 2 decrease temp:

1. CaCO3(s) <=> CaO(s) +CO2 (g) Delta H = +178 kJ/mol

Since Delta H is positive, it means the reaction is endothermic

a. An increase in temperature will will shift the equilibrium position to the right, thus forming more products

b. A decrease in the temperature will shift the equilibrium position to the left, thus forming more reactants

2. PCl3(g) + Cl2(g) <-> PCl5 (g) Delta H= -88 kJ/mol

From the above, Delta H is negative which implies exothermic reaction.

c. Increasing the temperature will shift the equilibrium position to the left, thus forming more reactants.

d. Decreasing the temperature will shift the equilibrium position to the right, thus forming more products

why is cellular respiration important for homeostasis?

it changes food into energy that the organism can use.

which of the following is most likely to happen if a cell is not able to divide?

the cell will not be replaced when it is damaged.

explanation:

fe 55.85 g/mol and h2o 18.02 g/mol.