Answer:
Explanation:
A 12.48 g sample of an unknown metal, heated to 99.0 °C was then plunged into 50.0 mL of 25.0 °C water. The temperature of the water rose to 28.1 Go to calculating final temperature when mixing two samples of water ... Problem #1: A 610. g piece of copper tubing is heated to 95.3 °C and placed in an ... The two rings are heated to 65.4 °C and dropped into 12.4 mL of water at 22.3 °C. ... Problem #4: A 5.00 g sample of aluminum (specific heat capacity = 0.89 J g¯1
– liquids, solids or gases – are made up of atoms and molecules that are in constant motion.<span> The theory also states that collisions between atoms and molecules are elastic</span>
Answer:
Explanation:
Heterogeneous mixtures: Milk, salt and pepper, smog, chocolate chip cookie, oil and water.
Solutions we might use everyday: Gatorade, Apple Juice, most wines and liquor, liquid detergent, coffee etc.
Answer:
According to Le Chatelier's principle, increasing the reaction temperature of an exothermic reaction causes a shift to the left and decreasing the reaction temperature causes a shift to the right.
Explanation:
C6H12O6(s) + 6O2(g) ⇌6CO2(g) + 6H2O(g)
We are told that the forward reaction is exothermic, meaning heat is removed from the reacting substance to the surroundings.
According to Le Chatelier's principle,
1. for an exothermic reaction, on increasing the temperature, there is a shift in equilibrium to the left and formation of the product is favoured.
2. if the temperature of the system is decreased, the equilibrium shifts to right and the formation of the reactants is favoured.
3. if the reaction temperature is kept constant, the system is at equilibrium and there is no shift to the right nor to the left.
<span>No, the denisty of any substance/liquid is always constant, no matter what the volume or mass is. Once the mass g/ volume mL is taken into consideration, the effect of the ammount of liquid given is canceled out. Thus, no matter what your sample is, the density of water will always be 1 g/mL</span>