E is the cell potential, E0is the standard cell potential, R is the gas constant, T is the temperature, n is the number of mole of electrons exchanged, F is Faraday's constant, and Q is the reaction quotient. The gas constant is equivalent to the Boltzmann constant, however, the gas ...
Calculate the volume, in liters, of 3.5 moles of H2S(g) at 70 degrees Celsius and 1.75 atm. Calculate the volume, in liters, of 5.15 moles of H2S(g) at 40 degrees Celsius and 1.75 atm. Calculate the volume, in liters, of 4.7...
V = Volume (Liters – L) n = Number of moles (mol) R = The Ideal Gas Constant (0.08206 L-atm/mol-K) T = Temperature (Kelvin)Ideal Gas Law Formula Questions: 1.) How many moles of gas are contained in 890.0mL at 21 °C and 750mm Hg? Answer: The Volume is V = 890.0mL an...
The unit atm (atmosphere) must always be used. V = Volume. This is always measured in liters n = number of moles of gas particles R = ideal gas constant = .08206 {eq}\frac{L atm}{ mol K} {/eq} T= temperature. This must always be measured with the Kelvin temperature scale ...
k is proportionality constant. V is the volume measured in liters. Answer and Explanation: Given values: The volume of the gas at initial state is V1=4.23 l. The pressure of the gas at initial state is {eq}P_1=\rm 2.25\...Become...
If 73.5 mol of an ideal gas is at 4.75 atm and 315 K, what is the volume of the gas? A sample of 5.0 moles of a gas at 1.0 atm is expanded at constant temperature from 10 L to 15 L. What is the final pressure? Calculate the volume of a gas, in liters, i...
6.2 liters of an ideal gas is contained at 3.0 atm and 37 °C. How manymolesof this gas are present? Solution The ideal gaslawstates PV = nRT Because the units of the gas constant are given using atmospheres, moles, and Kelvin, it's important to make sure you convert values given ...
V: Volume of the gas (ft3, m3, liter) n: Moles, or the number of molecules R: Gas universal constant, which is equal to 8.31 JKelvin.mol or 0.082 Litre.atmKelvin.molor 10.732 psift3Rankine.mol.pound T: Temperature of the gas in Rankine (R) or Kelvin (K) The pressure, temperature...
Boyle’s Law 3. A 2.50 m 3 of dry air, initially at 1.00 atm, is pumped into a rigid 50.0-L steel tank at constant temperature. What is the final air pressure in the tank? (Answer: 50.0 atm) 4. How many cubic meters of dry air, initially at 1.00 atm, must be pumped into a...
___Boyle’s Law 3.A 2.50 m 3 of dry air, initially at 1.00 atm, is pumped into a rigid 50.0-L steel tank at constant temperature. What is the final air pressure in the tank? (Answer: 50.0 atm) 4. How many cubic meters of dry air, initially at 1.00 atm, must be pum...