A student is investigating the affect of different salts on melting points. Four patches of ice of equal size are roped off and a different type of salt is poured on each, one receives table salt (NaCl), one receives Calcium Chloride (CaCl2), one receives Potassium Carbonate (KCO3) and the fourth receives inert sand instead. Each patch receives an equal amount of salt or sand. The student measures the volume of ice remaining and subtracts it from the original volume of ice to see how much melted away. What is the dependent variable?

A. The type of salt applied to the ice.
B. The size of the ice patches.
C. The amount of ice that melted.
D. The ice that received sand.

Answers

Answer 1

Answer:

Explanation:

A is the independent variable

D and B are control variables

Related Questions

PLEASE HELP QUICKLY!!!

HI gas is removed from the system
at equilibrium below. How does the
system adjust to reestablish
equilibrium?
51.8 kJ + H₂(g) + 1₂(g) = 2HI(g)
A. The reaction shifts to the right (products) and the concentrations
of I, and H₂ decrease.
B. The reaction shifts to the left (reactants) and the concentrations
of H₂ and I increase.
C. The reaction shifts to the right (products) and the concentrations
of I, and H₂ increase.
D. The reaction shifts to the left (reactants) and the concentration of
HI increases.

Answers

Answer:

A. The reaction shifts to the right (products) and the concentrations of I and H₂ decrease.

Explanation:

If gas is removed from the system at equilibrium, the system will try to compensate for the loss by shifting the reaction in a direction that produces more gas molecules. This is known as Le Chatelier's principle, which states that a system at equilibrium will respond to a disturbance by shifting in a way that minimizes the effect of the disturbance.

In this case, since gas is being removed from the system, the reaction will shift to the side that produces more gas molecules. Looking at the balanced equation, we can see that 2HI(g) has a greater number of gas molecules compared to H₂(g) and I₂(g). Therefore, the system will shift to the right (products) to produce more HI(g) and reestablish equilibrium.

if 500 mL of Ag+ solution contain 1.0 mols of Ag+, what is the molarity of the solution

Answers

Answer + explaination:

If 500 mL of Ag+ solution contain 1.0 mols of Ag+, what is the molarity of the solution

To calculate the molarity of the solution, we need to use the formula

Molarity = moles of solute / volume of solution in liters

We are given that the volume of the solution is 500 mL, which is the same as 0.5 L. We are also given that the solution contains 1.0 mole of Ag+.

Substituting these values into the formula, we get:

Molarity = 1.0 mol / 0.5 L = 2.0 M

Therefore, the molarity of the solution is 2.0 M.

Using the molarity formula, where molarity is equal to number of moles divided by volume(in liters) of the mixture is 2 mol/L.

Here, it is given that 500 mL of the Ag+ solution contains 1.0 mole of Ag+. To find molarity, the volume must first be converted to liters.

Solution volume = 500 mL = 500/1000 = 0.5 L

The molarity (M) can then be calculated using the following formula:

Molarity (M) equals moles of solute divided by the volume of solution (in liters).

Molarity = 1.0 mol / 0.5 L = 2.0 mol/L

As a result, the Ag+ solution has a molarity of 2.0 mol/L.

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Which of the following statements is true?
A.
Chemical reactions can either absorb thermal energy or release thermal energy.
B.
Chemical reactions can only release thermal energy.
C.
Chemical reactions can only absorb thermal energy.
D.
Chemical reactions can neither absorb thermal energy nor release thermal energy.

Answers

The answer is A, as all chemicals reactions exchange energy with the surroundings by releasing Or absorbing heat

Heat capacity of liquid water 4.18J/(g•k) Energy transferred?

Answers

The energy required to heat 1.00 g of water from 26.5°C to 83.7°C is 230 J. The energy formula for heating is, Energy = mcΔT.

Energy = mass × specific heat capacity × temperature change

Substituting the given values into the equation, we have:

Energy = 1.00 g × 4.18 J/(g·°C) × (83.7°C - 26.5°C) = 230 J

Therefore, the energy required is 230 J.

In this case, we are given the mass of water as 1.00 g and the specific heat capacity of water as 4.18 J/(g·°C).

The temperature change is 83.7°C - 26.5°C. By substituting these values into the equation, we find that the energy required is 230 J. This means that to heat 1.00 g of water from 26.5°C to 83.7°C, 230 J of energy must be supplied. The specific heat capacity is the amount of energy which is needed to increase the temperature of 1g of a substance by 1°C and in this case, it is 4.18 J/(g·°C) for water.

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Complete question:

The specific heat capacity of liquid water is 4.18 J/(g.k). How would you calculate the quantity of energy required to heat 1.00 g of water from 26.5 C to 83.7 C?

How do you balance

Ca(OH2) aq + H3PO4

In a neutralization equation?

Answers

Answer:

To balance this equation, we need two phosphate ions and three calcium ions. We end up with six water molecules to balance the equation: 2 H 3 PO 4 (aq) + 3 Ca (OH) 2 (aq) → 6 H 2 O (ℓ) + Ca 3 (PO 4) 2 (s) This chemical equation is now balanced.

Explanation:

Calculate the Kp for the following reaction at 25.0 °C:
H₂(g) + Br₂(g) 2 HBr (g)
Round your answer to 1 significant digit.
AG= -107
kJ
mol

Answers

The equilibrium constant for the reaction as it has been shown is [tex]5.7 * 10^{18}[/tex]

What is the equilibrium constant?

The quantitative expression of the size of a chemical process at equilibrium is the equilibrium constant, abbreviated as K. It links the reactant and product concentrations (or partial pressures) in a chemical process and gives details on the make-up of the equilibrium mixture. It offers crucial details regarding the proportions of reactants and products.

We know that;

ΔG = -RTlnKp

Thus we have that;

Kp =[tex]e^-[/tex](ΔG/RT)

Kp = [tex]e^-[/tex](-107000 /8.314 * 298)

=[tex]5.7 * 10^{18}[/tex]

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