Explain why the changes shown are physical change
Answers
The changes shown are physicalchanges because when ice melts, it turns from solid to liquid.
What are physical changes?
Physical changes are when a substance changes in how it looks or acts without turning into something else. These changes can usually be undone, which means the substance can be brought back to how it was before.
When ice melts, it turns from solid to liquid. The tiny particles in the ice move around, but the stuff that makes up water stays the same. The process can go backwards, because the water that is a liquid can be turned back into ice.
When water gets really hot, it turns into gas called steam. The water molecules get enough energy to separate from each other and become vapor. Once again, the stuff that makes up water stays the same, and when steam cools down, it turns back into liquid water.
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Answer:
Because physical change are reversible change. we can reverse into the orginal effect.
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Red blood cells are formed in the bone marrow of the _______
Answers
Answers
Tetra phosphorous octa bromide is the compound name for P4Br8.
What is compound?
A substance is from a combination of two or more different chemical elements. They are pure chemical substances found in nature.
- The smallest unit of a compound is molecule.
- Both phosphorous and bromide are on the right side of the periodic table.
- Both phosphorous and bromide form covalent bond.
- Atomic weight of phosphorous is 30.97 and atomic number is 15.
- Atomic weight of bromine is 79.9 and atomic number is 35.
The name is tetra because there are 4 phosphorous and octa means there is 8 bromide.
The ratio of phosphorous and bromide is 4:8.
Tetra phosphorous octa bromide is the compound name for P4Br8.
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14/7N + ____ ---> 14/6C + 1/1H
Answers
Explanation:
The given reaction equation is as follows.
+ ___
As there is release of one hydrogen which shows that mass number has increase by 1 on the product side.
Therefore, particle must be added in order to balance the given reaction equation.
Hence, the complete reaction equation will be as follows.
Final answer:
To complete the nuclear reaction equation, the particle required is a neutron (1/0n). It's calculated based on the law of conservation of mass and atomic numbers in nuclear reactions.
Explanation:
To complete the nuclear reaction equation 14/7N + ____ ---> 14/6C + 1/1H, we need to conserve both the mass number (the sum of protons and neutrons) and atomic number (number of protons). On the left side of the equation, we have nitrogen (represented by 14/7N), with a mass number of 14 and atomic number of 7. On the right side, Carbon (14/6C) has atomic number 6 and a mass number of 14 and Hydrogen (1/1H) has atomic number 1 and a mass number of 1. So, to balance the equation we need an element with atomic number (7-6-1) = 0 and mass number (14-14-1) = -1. This element is a neutron (represented as 1/0n), as it has a mass number of 1 and atomic number of 0.
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Hope this helped and if you need more help then just message me instead ok m:)
3. The appearance of the offspring is referred to as
4. The genetic make-up of the genes of the offspring is
5. Having two identical alleles of a particular gene or genes is called
6. The father of Science of Genetic is
7. It is the trait that is being expressed in an organism.
8. The extent to which something is probable is
9. The offspring of two plants/animals of different species or varieties is called
10. It is the number of times that the genotype would appear in an offspring after a test cross is
11. The relative number of offspring manifesting a particular trait or a combination of traits.
12. Having two different alleles of a particular gene or genes is
Answers
Answer:
1-Genetics
2-Alleles
3-Organism's genotype
4-Phenotypes and Genotypes
5-Allele
6-Gregor Mendel
7-Genotype
8-Probability
9-Hybrid
10-Genotypic Ratio
11-Phenotypic ratio
12-Heterozygous
Explanation:
3. What temperature (in °C) did an ideal gas shift to if it was initially at -17.00 °C at 4.620 atm and 35.00 L and the pressure was changed to 8.710 atm and the volume changed to 15.00 L?
4. A mixture of two gases with a total pressure of 1.98 atm contains 0.70 atm of Gas A. What is the partial pressure of Gas B in atm?
5. A chamber contains equal molar amounts of He, Ne, Ar, and Kr. If the total chamber pressure is 1 atm, then the partial pressure (in atm) of Kr is:
Answers
Answer:
1. To find the volume of 8.20 moles of CO₂ at standard temperature and pressure (STP), we can use the ideal gas law. At STP, the temperature is 0 °C or 273.15 K, and the pressure is 1 atm. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
We can rearrange the equation to solve for V:
V = (nRT) / P
Substituting the values:
V = (8.20 mol * 0.0821 L·atm/mol·K * 273.15 K) / 1 atm
Calculating the numerical value:
V ≈ 181.3 L
Therefore, the volume of 8.20 moles of CO₂ at STP is approximately 181.3 liters.
2. To find the pressure of a gas sample with 3.05 moles in a 10.00 L container at 45.0 °C, we can still use the ideal gas law. However, we need to convert the temperature to Kelvin by adding 273.15 to it.
The ideal gas law equation can be rearranged to solve for pressure:
P = (nRT) / V
Substituting the values:
P = (3.05 mol * 0.0821 L·atm/mol·K * (45.0 + 273.15) K) / 10.00 L
Calculating the numerical value:
P ≈ 4.083 atm
Therefore, the pressure of the gas sample is approximately 4.083 atm.
3. To find the final temperature in °C when the initial temperature was -17.00 °C, and the pressure changed from 4.620 atm to 8.710 atm, and the volume changed from 35.00 L to 15.00 L, we can use the combined gas law.
The combined gas law states that (P₁ V₁) / T₁ = (P₂ V₂) / T₂, where P is pressure, V is volume, and T is temperature.
Rearranging the equation to solve for T₂:
T₂ = (P₂ V₂ T₁) / (P₁ * V
Final answer:
The volume of 8.20 moles of CO₂ at standard temperature and pressure (STP) is approximately 180.4 liters.
Explanation:
Gas Laws
Gas laws describe the behavior of gases under different conditions. One of the fundamental gas laws is the ideal gas law, which relates the pressure, volume, temperature, and number of moles of a gas. The ideal gas law equation is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Question 1: Volume of CO₂ at STP
To find the volume of 8.20 moles of CO₂ at standard temperature and pressure (STP), we can use the ideal gas law equation. At STP, the temperature is 0 degrees Celsius (273.15 Kelvin) and the pressure is 1 atmosphere (atm).
Given:
- Number of moles (n) = 8.20 moles
- Temperature (T) = 0 degrees Celsius (273.15 Kelvin)
- Pressure (P) = 1 atmosphere (atm)
Using the ideal gas law equation, we can rearrange it to solve for the volume (V):
V = (nRT) / P
Substituting the given values:
V = (8.20 moles * 0.0821 L·atm/mol·K * 273.15 K) / 1 atm
V ≈ 180.4 liters
Question 2: Pressure of Gas
To find the pressure of a gas in a given container, we can use the ideal gas law equation. The temperature must be converted to Kelvin before using the equation.
Given:
- Number of moles (n) = 3.05 mol
- Volume (V) = 10.00 L
- Temperature (T) = 45.0 °C (318.15 Kelvin)
Using the ideal gas law equation, we can rearrange it to solve for the pressure (P):
P = (nRT) / V
Substituting the given values:
P = (3.05 mol * 0.0821 L·atm/mol·K * 318.15 K) / 10.00 L
P ≈ 7.79 atm
Question 3: Temperature Change
To find the temperature change of an ideal gas, we can use the ideal gas law equation. The initial and final conditions of the gas must be known.
Given:
- Initial temperature (T1) = -17.00 °C (256.15 Kelvin)
- Initial pressure (P1) = 4.620 atm
- Initial volume (V1) = 35.00 L
- Final pressure (P2) = 8.710 atm
- Final volume (V2) = 15.00 L
Using the ideal gas law equation, we can rearrange it to solve for the final temperature (T2):
T2 = (P2 * V2 * T1) / (P1 * V1)
Substituting the given values:
T2 = (8.710 atm * 15.00 L * 256.15 K) / (4.620 atm * 35.00 L)
T2 ≈ 303.6 °C
Question 4: Partial Pressure of Gas B
To find the partial pressure of Gas B in a mixture of gases, we need to know the total pressure and the partial pressure of Gas A.
Given:
- Total pressure = 1.98 atm
- Partial pressure of Gas A = 0.70 atm
The partial pressure of Gas B can be calculated by subtracting the partial pressure of Gas A from the total pressure:
Partial pressure of Gas B = Total pressure - Partial pressure of Gas A
Partial pressure of Gas B = 1.98 atm - 0.70 atm
Partial pressure of Gas B ≈ 1.28 atm
Question 5: Partial Pressure of Kr
To find the partial pressure of Kr in a chamber containing equal molar amounts of He, Ne, Ar, and Kr, we need to know the total chamber pressure.
Given:
- Total chamber pressure = 1 atm
Since the chamber contains equal molar amounts of gases, the partial pressure of Kr is equal to the total chamber pressure divided by the number of gases:
Partial pressure of Kr = Total chamber pressure / Number of gases
Partial pressure of Kr = 1 atm / 4
Partial pressure of Kr = 0.25 atm
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