Answer:
B. 92.4 g
Explanation:
the balanced equation for the reaction is as follows
CaCO₃ + 2HCl ---> CaCl₂ + CO₂ + H₂O
molar ratio of CaCO₃ to CaCl₂ is 1:1
number of CaCO₃ moles reacted - 104 g / 100 g/mol = 1.04 mol
therefore number of CaCl₂ moles reacted - 1.04 mol
mass of CaCl₂ expected to be formed = 1.04 mol x 111 g/mol = 115.44 g
percentage yield = actual yield / theoretical yield x 100 %
theoretical yield = 115.44 g
percentage yield = 80.15 %
substituting these values in the above equation
80.15 % = actual yield / 115.44 g x 100 %
actual yield = 92.5 g
therefore answer is B. 92.4 g
Answer:
The correct answer is "single replacement".
Explanation:
The activity series is a representation of a series of metals that are organized according to their order of reactivity. They start from the highest order of reactivity to the lowest order of reactivity.
The purpose of the series is to determine which products are formed in single-displacement reactions. The higher-order metals replace the lower order metals if there are two of them in the same solution. If metal is higher in the series it is more reactive than a metal that is below it in the activity series.
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Introduction:
Understanding the amount of energy required to change the temperature of a substance is fundamental in many fields, from chemistry and physics to engineering and everyday applications. In this case, we're looking at how much energy it takes to heat a 75 g sample of aluminum.
Specific Heat Capacity of Aluminum:
To determine the energy required, we first need to consider the specific heat capacity of aluminum. The specific heat capacity (c) is a unique property of each material and represents the amount of heat energy needed to raise the temperature of 1 gram of that substance by 1 degree Celsius (or 1 Kelvin). For aluminum, the specific heat capacity (c) is approximately 0.897 J/g°C (joules per gram per degree Celsius).
Mass of the Sample:
The next piece of the puzzle is the mass of the aluminum sample. You mentioned that it's 75 grams, so we'll use that value in our calculations.
Change in Temperature:
We're looking to raise the temperature of the aluminum from 22.4°C to 94.6°C. To find the change in temperature (ΔT), we subtract the initial temperature from the final temperature:
ΔT = 94.6°C - 22.4°C = 72.2°C
Calculating the Energy:
Now, we can use the specific heat capacity formula to calculate the energy (Q) needed to raise the temperature of the aluminum sample:
Q = m * c * ΔT
Where:
Q is the energy in joules (J).
m is the mass of the sample (75 g).
c is the specific heat capacity of aluminum (0.897 J/g°C).
ΔT is the change in temperature (72.2°C).
Plugging in these values:
Q = 75 g * 0.897 J/g°C * 72.2°C
Q ≈ 4863.15 J
Conclusion:
Therefore, approximately 4863.15 joules of energy are needed to raise the temperature of a 75 g sample of aluminum from 22.4°C to 94.6°C. This calculation is essential in various scientific and practical applications, from cooking to materials engineering, and helps us understand the energy requirements for temperature changes in different substances.
Answer:
true
true
Explanation:
pki points nmn po
Answer:
A
An acid and a base
Explanation:
B. An ionized atom has a number of protons that is unequal to the number of electrons.
C. A cation will hold a positive charge if it gains one or more electrons.
D. Losing one or more electrons will turn an atom into an anion.
Answer:
B. An ionized atom has a number of protons that is unequal to the number of electrons.
Explanation:
Bc its is got 100% on pf