305 k
Using Charles's Law (V1/T1 = V2/T2), we can solve for the final temperature: (1400/83) = (1200/T2). Rearranging gives: T2 = (1200 * 83) / 1400 β 71.4 Β°C.
0.50 moles of NH3 at STP (Standard Temperature and Pressure) occupies 11.2 liters of volume.
1 mole of gas particles at STP (Standard Temperature and Pressure) occupies a volume of 22.4 liters.
The amount of space that a sample of matter occupies is called its volume. This can be measured in units such as cubic meters, liters, or cubic centimeters depending on the scale of the sample.
The volume of 0.8 moles of a gas at Standard Temperature and Pressure (STP) is 17.6 liters. This is because at STP, one mole of any ideal gas occupies 22.4 liters.
Using the ideal gas law equation, we can calculate the new volume of the gas. At STP, the pressure is 1 atm, which means 50 atm is 50 times greater. So the new volume would be 1.55L / 50 = 0.031L, when the pressure is increased to 50 atm.
To find the new volume, you can use the combined gas law formula: (P1 * V1) / T1 = (P2 * V2) / T2. Since pressure is constant, it can be eliminated. Rearrange the formula to solve for V2: V2 = (V1 * T2) / T1. Plug in the values: V2 = (20 ml * 323 K) / 141 K = 45.1 ml. So, the sample of gas would occupy 45.1 ml at 50 C.
To find the new volume, we can use the Charles's Law equation: V1 / T1 = V2 / T2. Plugging in the values, we get 3.8 / (-45 + 273) = V2 / (45 + 273). Solving for V2 gives us approximately 4.22 liters.
423mL
Using the ideal gas law equation, we can calculate the new volume of the gas. At STP, the pressure is 1 atm, which means 50 atm is 50 times greater. So the new volume would be 1.55L / 50 = 0.031L, when the pressure is increased to 50 atm.
419 mL
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
129
Volume is a measure of how much space a sample of matter occupies. the SI unit of volume is m3 .
A sample of Ar gas occupies a volume of 1.2 L at 125Β°C and a pressure of 1.0 atm. Determine the temperature, in degrees Celsius, at which the volume of the gas would be 1.0 L at the same pressure.
Volume = how much space an object occupies, that nothing else can occupy at the same time.
It depends on temperature and pressure. Assuming 25.0ºC and 1.00 atmospheres then 125 g CO2 occupies 54.7 dm3.
0.667