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Using the ideal gas law (PV = nRT), we can calculate the number of moles of air in the balloon at the initial conditions. Then, using the new temperature and the same number of moles, we can calculate the final volume of the air in the balloon. The final volume will be less than 5.5 L due to the decrease in temperature.
The volume of a balloon is proportional to the pressure it is under, so if the volume is 6 cubic inches at 99 feet, it would have a different volume at 33 feet. To find the new volume at 33 feet, you would need to use Boyle's Law, which states that the initial pressure times the initial volume equals the final pressure times the final volume. So, you would use the formula P1V1 = P2V2 to solve for the new volume at 33 feet.
The density decreases by half. You find the answer by knowing that density is equal to mass divided by the volume. If the mass stays constants and the volume is doubled, then the density is halved.
Using the ideal gas law, we can calculate the new volume of the balloon. Given that the initial volume is 0.75 L, the initial temperature is 25°C (298 K), and the final temperature is -100°C (173 K), we can use the equation (V1/T1) = (V2/T2) to find the new volume. Plugging in the values, we get V2 = (0.75 L * 173 K) / 298 K ≈ 0.44 L.
The volume of air increases proportionally as it is heated, according to the formula: PV/T = P'V'/T' Where P, V, and T are initial values for pressure, volume and temperature in absolute terms and P',V',and T' are the final values with a constant pressure the equation becomes: V/T = V'/T' to solve for final volume the equation is: VT'/T = V' if V=1cu. meter, T = 200K and T' = 300K then 1 cu.meter x 300K/200K = 1.5 cu.meter
Using the ideal gas law (PV = nRT), we can calculate the number of moles of air in the balloon at the initial conditions. Then, using the new temperature and the same number of moles, we can calculate the final volume of the air in the balloon. The final volume will be less than 5.5 L due to the decrease in temperature.
Change Celsius to Kelvin by adding 273.15. 25 C = 298.15 K 50 C = 323.15 K An equality. 500.0 ml/298.15 K = X ml/323.15 K 298.15X = 161575 X = 541.925 milliliters -------------------------------you do significant figures
To find the new volume of the balloon, you can use the ideal gas law formula: V2 = V1 * (T2/T1), where V1 is the initial volume (45L), T1 is the initial temperature (25°C), and T2 is the final temperature (55°C). Plugging in the values, V2 = 45 * (55/25) = 99L. So, the new volume of the balloon would be approximately 99 liters.
The way to keep this simple is to assume that the pressure in the balloon remains constant throughout the operation. The only trick to this whole thing is to understand that-- At constant pressure, volume is directly proportional to temperature.Volume2/Volume1 = Temperature2/Temperature1-- 'Temperature' means absolute temperature ... Kelvin, or (Celsius + 273).? The initial temperature of 20 C is absolute temp of 293 K.If the pressure remains constant, thenAbsolute-temp2 = Absolute-temp1 x (Volume2/Volume1) = 1,000 x 293/750 = 3902/3 K.°Celsius = Absolute - 273 = 117 2/3 ° C.
If the initial volume is smaller than the final volume, this suggests that there has been an increase in volume. This could be due to factors such as expansion of a substance when heated, addition of more material, or a phase change from a more condensed state to a less condensed state.
The volume of a balloon is proportional to the pressure it is under, so if the volume is 6 cubic inches at 99 feet, it would have a different volume at 33 feet. To find the new volume at 33 feet, you would need to use Boyle's Law, which states that the initial pressure times the initial volume equals the final pressure times the final volume. So, you would use the formula P1V1 = P2V2 to solve for the new volume at 33 feet.
The density decreases by half. You find the answer by knowing that density is equal to mass divided by the volume. If the mass stays constants and the volume is doubled, then the density is halved.
Using the ideal gas law, we can calculate the new volume of the balloon. Given that the initial volume is 0.75 L, the initial temperature is 25°C (298 K), and the final temperature is -100°C (173 K), we can use the equation (V1/T1) = (V2/T2) to find the new volume. Plugging in the values, we get V2 = (0.75 L * 173 K) / 298 K ≈ 0.44 L.
The volume of air increases proportionally as it is heated, according to the formula: PV/T = P'V'/T' Where P, V, and T are initial values for pressure, volume and temperature in absolute terms and P',V',and T' are the final values with a constant pressure the equation becomes: V/T = V'/T' to solve for final volume the equation is: VT'/T = V' if V=1cu. meter, T = 200K and T' = 300K then 1 cu.meter x 300K/200K = 1.5 cu.meter
Assuming that none of the solid evaporated during the time that it was being heated, then the mass must be conserved. Then, assuming that after the object is in its' final shape the density of the material returns to its' original value the volume must be unchanged. This is because mass = volume * density. However, the surface area does not have to be the same.
(v1/t1) = (v2/t2)
To find the final concentration of a solution after dilution, you can use the formula: (C_1V_1 = C_2V_2), where (C_1) is the initial concentration, (V_1) is the initial volume, (C_2) is the final concentration, and (V_2) is the final volume. Plug in the values for the initial concentration, volume, and final volume to calculate the final concentration of HCl.