Which of the following is TRUE about a physical change in matter?O A physical change changes the identity of the substance
O A physical change does not change the chemical formula of the substance
O A physical change has similar characteristics as a chemical change.
A physical change is a change in how the substances react with other substances.

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

Learn more about gas laws here:

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Answer:

1.88 x 10^5

Explanation:

You have to round because all of the numbers in 187515.4207 are significant

Round to: 188000

Put in scientific notation:

1.88 x 10^5

Answer:

well scientific notation would be = 1.875154207 × 10^5

you cant rlly simply the number any further to get 3 sig figs

youd need something like 187 to be 3 sig figs

are you saying the question correctly?