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No. As long as you don't take any of it away, the same quantity of mass is
still there, and the same quantity of mass always has the same weight,
regardless of what physical state it happens to be in.
No, the weight of the water remains unchanged. Mass is conserved. It does, however, become less dense (takes up a little bit more volume).
What else can I help you with?
When urea is added to water the freezing point is decrease why?
This is a colligative property. Adding a solute will increase the boiling point and decrease the freezing point. The reason has to due with intermolecular forces, and interruption thereof. When water molecules have solute in between them, the temperature has to be lower than normal in order for them to freeze.
What describes the change in the mass of water during the freezing process does it stay the same?
During the freezing process, the mass of water remains the same. While the water changes from liquid to solid form, the amount of water does not increase or decrease; it merely undergoes a phase change. Therefore, the total mass of the water before and after freezing is constant.
A solution of glucose in water has a freezing point that is?
A solution of glucose in water has a freezing point that is lower than that of pure water due to the presence of solute particles, which disrupt the formation of ice. This phenomenon is known as freezing point depression. The extent of the freezing point depression depends on the concentration of glucose in the solution, as more solute particles lead to a greater decrease in the freezing point.
Is water freezing an example of an endothermic reaction?
No, water freezing is not an endothermic reaction; it is an exothermic process. During freezing, water releases heat to its surroundings as it transitions from a liquid to a solid state. This release of energy is what causes the temperature of the surroundings to decrease. In contrast, an endothermic reaction absorbs heat from the environment.
How does elevation effect freeze point?
As elevation increases, the atmospheric pressure decreases. This causes the boiling point of water to decrease, but the freezing point remains relatively unaffected. Therefore, elevation does not significantly impact the freezing point of water.
What results in decrease in entropy?
Water Freezing
What result in a decrease in entropy?
water freezing
Would result in a decrease in entropy?
water freezing
How much would the freezing point of water decrease if 4 moles of Na-Cl were added to 1 Kg of water?
The freezing point decrease is -14,8 oC.
How does salt affect the water's melting point?
Adding salt to water the freezing point decrease.
How would the freezing point of water decrease if 4 mol of NaCl were added to 1kg of water?
The freezing point of water would decrease if 4 mol of NaCl were added because NaCl is a solute that disrupts the water molecules' ability to form solid ice. Each mole of NaCl added to water reduces the freezing point by approximately 1.86 degrees Celsius. So, with 4 mol of NaCl added, the freezing point of water would decrease by about 7.44 degrees Celsius.
How much Would the freezing point of water decrease of sugar were added to 1 kg of water?
The freezing point of water decreases by about 1.86 degrees Celsius for each mole of solute (such as sugar) dissolved in 1 kg of water. So, the freezing point would decrease by 1.86 degrees Celsius for every mole of sugar added.
How much would the freezing point of water decrease if 4 mol of sugar were added to 1kg of water?
The normal freezing temperature for pure water is 0c. Howeverif sugar is added in the pure water, the freezing point will be lower than zero. How far below zero will depend on the sugar concentration in the water.
Why is salt not good for melting ice?
Adding a salt the freezing point of water decrease.
Why doesn't the temperature of water continue to decrease once it hits freezing point?
It freezes
When starch is stirred into water will it increase or decrease the boiling or freezing point?
There is hardly any change
How much would the freezing point of water decrease if 4 mol of nacl were added to 1 kg of water?
The freezing point of a solution decreases according to the formula: delta Tf = Kf * molality. Given that the molality of the solution is 4 moles NaCl per kg water and the Kf value for water is 1.86 °C/m, the decrease in freezing point would be approximately 7.44°C.
