Answer:
The volume of the container would be 1507 L
Explanation:
These question can be solved in two different ways:
Let's do the short road.
We know that 1 mol of anything at STP conditions occupies 22.4 L
By a rule of three:
1 mol contains 22.4L at STP
Then, 67.3 mol of gas would be contained in (67.3 . 22.4) /1 = 1507.5 L
We assume CO₂ as an Ideal Gas, so we can apply P . V = n . R . T
At STP, T is 273.15K and P = 1 atm. We replace:
1 atm . V = 67.3 mol . 0.082 . 273.15K
V = (67.3 mol . 0.082 . 273.15K) / 1 atm → 1507 L
In an endothermic reaction products are <u>HIGHER </u>than reactants in potential energy and <u>LESS </u>stable.
Explanation:
Energy is input into the reaction in an endothermic reaction. This means the products are of a higher energy level than the reactants. Therefore the reaction increases Gibb's free energy and reduces entropy. Remember in thermodynamic stability involves an increase in entropy and a decrease in Gibbs free energy. Therefore the products are less stable than the reactants. This is why endothermic reactions do not occur spontaneously like exothermic reactions.
Answer:
17.3 g
Explanation:
<u>Given the following data;</u>
- Quantity of heat, Q = 0.507 J
- Temperature = 0.007°C
- Specific heat capacity of water = 4.2 J/g°C
Mathematically, Heat capacity is given by the formula;
Where;
- Q represents the heat capacity or quantity of heat.
- M represents the mass of an object.
- C represents the specific heat capacity of water.
- T represents the temperature.
Making "M" the subject of formula, we have;
Substituting the values into the formula, we have;
<em>Mass, m = 17.3 grams</em>