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What is the equation to the reaction of blowing up an balloon?
The reaction of blowing up a balloon involves the expansion of air, which can be described using the ideal gas law: ( PV = nRT ). Here, ( P ) represents the pressure of the air inside the balloon, ( V ) is the volume of the balloon, ( n ) is the number of moles of air, ( R ) is the ideal gas constant, and ( T ) is the temperature in Kelvin. As air is blown into the balloon, the volume increases, leading to changes in pressure and temperature within the balloon.
If a large balloon contains 224 liters of gas at STP then there is 100 mole of gas in the balloon How many moles of gas are in a balloon that is 560 liters at STP?
Using the ideal gas law, at STP (standard temperature and pressure), 1 mole of gas occupies 22.4 liters. Therefore, a balloon with 560 liters at STP would contain 25 moles of gas (560 liters / 22.4 liters/mole).
What is the density of Cl2 gas at STP?
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
How many moles is 15.2L of CH4?
It depends on temperature,pressure and volume.THese are needed to find number of moles
What is the pressure in a 0.34 L balloon if the temperature is 35C and the balloon contains 0.0233 mol of an ideal gas?
Using the ideal gas law, PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin, we can calculate the pressure. First, convert the temperature to Kelvin by adding 273.15: 35C + 273.15 = 308.15K. Then, plug in the values: P = (0.0233 mol) * (0.0821 L atm/mol K) * (308.15K) / 0.34L. This gives a pressure of approximately 1.94 atm.
Does a balloon show that air can be compressed?
Yes, a balloon shows that air can be compressed. The pressure in the balloon is higher than the pressure outside the balloon. The ideal gas law is PV = nRT where: P = pressure V = volume n = the number of moles of gas (the amount of gas) R = the ideal gas constant T = temperature So for the given volume of the balloon, and at a set temperature, if the pressure goes up, the amount of gas (the number of moles) must also go up. That means that the gas has been compressed.
What is the equation to the reaction of blowing up an balloon?
The reaction of blowing up a balloon involves the expansion of air, which can be described using the ideal gas law: ( PV = nRT ). Here, ( P ) represents the pressure of the air inside the balloon, ( V ) is the volume of the balloon, ( n ) is the number of moles of air, ( R ) is the ideal gas constant, and ( T ) is the temperature in Kelvin. As air is blown into the balloon, the volume increases, leading to changes in pressure and temperature within the balloon.
When balloon put into a hot water what will happens to the molecules inside?
The ideal gas law is pv=nrt. p=pressure v=volume n=moles r=a gas constant t=temperature When a balloon full of air (a gas) is heated the temperature rises. We know that r and n are constant so all we have to look at the relationship between temperature and pressure/volume. t~p and t~v Therefore as temperature goes up pressure and volume will both go up. How much however one will change over the other is a function of the tensile strength of the balloon and beyond the scope of this answer.
How many moles of helium will a 75.0-L balloon hold if a 27.5-L balloon holds 1.76 moles at the same temperature and pressure?
Using the ideal gas law, we can calculate the number of moles in the 75.0-L balloon by setting up a proportion using the volume and moles relationship between the two balloons. By cross-multiplying, we find that the 75.0-L balloon will hold approximately 4.85 moles of helium.
A balloon contains 5.5 L of air at 303 K and 101.3 kPa After an hour the air inside the balloon cools to 297 K What is the final volume of the air in the balloon?
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.
What is the volume of a balloon at STP if it holds 5.00 moles of gas?
At Standard Temperature and Pressure (STP), the volume of 1 mole of gas is 22.4 L. Therefore, if the balloon holds 5.00 moles of gas at STP, the volume would be 5.00 moles x 22.4 L/mole = 112 L.
If a large balloon contains 224 liters of gas at STP then there is 100 mole of gas in the balloon How many moles of gas are in a balloon that is 560 liters at STP?
Using the ideal gas law, at STP (standard temperature and pressure), 1 mole of gas occupies 22.4 liters. Therefore, a balloon with 560 liters at STP would contain 25 moles of gas (560 liters / 22.4 liters/mole).
When is pressure useful?
when determining volume, moles, weight, and/or temperature
What is the density of Cl2 gas at STP?
what is the volume of a balloon containing 50.0 moles of O2 gas at a pressure of 15.0 atm at 28 degrees
The volume of a gas is directly proportional to the number of moles of that gas if?
the pressure and temperature are held constant. ideal gas law: Pressure * Volume = moles of gas * temperature * gas constant
What is the relationship between temperature, volume, pressure, and the number of moles of a gas as described by the ideal gas law equation w-nRT?
The ideal gas law equation, w-nRT, describes the relationship between temperature (T), volume (V), pressure (P), and the number of moles of a gas (n). It states that the product of pressure and volume is directly proportional to the product of the number of moles, the gas constant (R), and the temperature. In simpler terms, as temperature increases, the volume of a gas increases if pressure and the number of moles are constant. Similarly, if pressure increases, volume decreases if temperature and the number of moles are constant.
How many moles is 15.2L of CH4?
It depends on temperature,pressure and volume.THese are needed to find number of moles
