Answer:
See explanation
Explanation:
According to the kinetic molecular theory, the molecules that compose a gas are in constant random motion.
The temperature of a gas is a measure of the average kinetic energy of the gas molecules.
When the balloon was placed in a hot water bath, the balloon becomes larger because the gas inside the balloon expands. This is because, more kinetic energy is supplied to the molecules of the gas hence they spread out.
When the balloon is placed in cold water, the kinetic energy of the gas molecules in the balloon decreases as temperature decreases hence the balloon shrinks
Exothermic type of reaction is taking place because this type of reaction generates heat energy.
<h3>What is exothermic reaction?</h3>
Exothermic reactions refer to those chemical reactions that produce heat energy and release that heat energy to the surrounding environment.
So we can conclude that exothermic type of reaction is taking place because this type of reaction generates heat energy.
Learn more about reaction here: brainly.com/question/26018275
Super saturated solution is formed.
<u>Explanation:</u>
Solubility is the property of any substance's capacity, that is the solute of the substance is dissolved in the given solvent to form the solution. We have three different types of solution, unsaturated, saturated and supersaturated solution.
- Unsaturated solution is a solution with lesser amount of solute than its solubility at equilibrium.
- Saturated solution is a solution with the maximum solute dissolved in the solvent.
- Super saturated solution is a solution with more solute than it is required.
The solubility of KI at 30°C is 153 g / 100 ml. Here 180 g of KI in 100 ml of water at 30°C is given, which has more solute than required, so it is super saturated solution.
Answer:
The answer is D all of the above
Explanation:
Answer:
44.62 kJ
Explanation:
Firstly, we calculate the energy needed to heat the liquid (ethyl alcohol) by using the formula:
Q = m × c × ∆T
Where;
Q = Amount of heat (J)
m = mass (g)
c = specific heat of ethyl alcohol = 2.138 J/g°C
∆T = change in temperature (°C)
According to the information given in this question;
Q = ?, m = 50.0g, ∆T = (78.4°C - 60°C) = 18.4°C
Therefore, using Q = mc∆T
Q = 50 × 2.138 × 18.4
Q (amount of energy needed to heat ethyl alcohol) = 1966.96 J
Next, we calculate and add the amount of heat needed to vaporize by using the formula;
How many kilojoules of energy are required to heat 50.0 g of ethyl alcohol from 60.0 °C to 78.4 °C and vaporize it? The specific heat of ethyl alcohol is heat of vaporization is 853 J/g.
