Ideal Gas Equation help!?
PV = nRT T = PV / (nR) you need to make sure your units match up.. P = 100,000 Pa V = 0.000268 m³ n = 0.0084 moles R = 8.31 m³ Pa / mole K T = (100,000 Pa) x (0.000268 m³) / [( 0.0084 moles) x (8.31 m³ Pa / mole K)] T = 384 K = 384 - 273 °C = 111 °C notice that all the units canceled except for K?
Ideal Gas Equation help?
n = PV/RT = 0.986 atm x 0.112 L / (0.08206 x 373) = 0.00361 mole 0.109 g / 0.00361 mole = 30.2 g/mole
Ideal Gas Equation help!?
10. Mg + 2 HCl → MgCl2 + H2 PV = nRT n = PV / RT = (100 kPa) x (0.100 L) / ((8.3144621 L kPa/K mol) x (298 K)) = 0.0040360 mol H2 (0.0040360 mol H2) x (1 mol Mg/ 1 mol H2) x (24.30506 g Mg/mol) = 0.0981 g Mg (0.0040360 mol H2) x (2 mol HCl / 1 mol H2) / (2.0 mol/dm^3) = 0.0040 dm^3 HCl 11. 2 Na + 2 H2O → H2 + 2 NaOH (0.52 g Na) / (22.98977 g Na/mol) = 0.02262 mol Na (100 g H2O) / (18.01532 g H2O/mol) = 5.55 mol H2O Clearly H2O is in large excess, so Na is the limiting reactant. (0.02262 mol Na) x (1 mol H2 / 2 mol Na) = 0.01131 mol H2 a) PV = nRT V = nRT / P = (0.01131 mol H2) x (8.3144621 L kPa/K mol) x (298 K) / (100 kPa) = 0.28 L H2 b) (0.02262 mol Na) x (2 mol NaOH / 2 mol Na) / (0.100 L) = 0.23 mol/L
Ideal Gas Equation help?
Acetylene gas, C2H2(g), can be prepared by the reaction of calcium carbide with water CaC2(s)+2H2O(l)-->Ca(OH)2(aq)+C2H2(g) Calculate the volume of C2H2 that is collected over water at 23 degrees C by reaction of 1.524g of CaC2 if the total pressure of the gas is 753 torr. Vapor pressure of water =21.07 torr
Please help with this Ideal Gas equation!?
You can start by working out how many moles of N2 will be 26.5L. you can put all of the values into the ideal gas equation pV=nRt where: p=110000 pa V=26.5/1000 (m^3) R=8.31 t=273+22=295 (K) and then rearrange to find out the value of n (number of moles) once you know this, you can divide it by 3 to work out the number of moles of each element (before it is multiplied by the number in from (coefficient)) and then multiply it by 2 to work out the number of moles of 2NaN3. Once you know this you can work out the Mr of it to be (23+14x3)x2=130. and then you multiply 130 by the number of moles to get the mass in grams. I hope you can follow this and if you get confused then I recommend looking at some youtube videos on using the ideal gas equation with examples until you fully understand it.
Ideal Gas Equations help?
Values for the ideal gas constant R for different pressure units. a. If the pressure is measured in kPa then R = 8.31 kPa. – L / mol – K b. If the pressure is measured in atm then R = 0.082 atm. – L / mol – K c. If the pressure is measured in mm or torr then R = 62.4 torr. – L / mol – K d. If the pressure is measured in p.s.i. then R = 1.21 kPa. – L / mol – K 1. Calculate the volume of 1.53 moles of helium gas at 24.0C and 633 mmHg. 2. How many moles are contained in 1250 mL of oxygen gas at 19.0 Celsius and 14.2 psi ? 3. What is the volume of 2.35 moles of any ideal gas at 26.0 Celsius and 83.2 kPa ? 4. What is the temperature in Celsius of 0.7638 grams of oxygen gas occupying a volume of 500.0 mL at a pressure of 1.07 atm ? 5. Calculate the pressure of 9.53 moles of helium gas at 273 K. and a volume of 2.4 L 8 How many moles are contained in 5.00 L of oxygen gas at 419.0 Celsius and 26.8 psi ? 9. What is the volume of 0.55 moles of any ideal gas at 45.0 Celsius and 99.2 kPa ? 10. What is the temperature in Celsius of 2.76 grams of oxygen gas occupying a volume of 2.66 L at a pressure of 1.07 atm ? 11. What is the pressure of 4.66 moles of gas at 300 K occupying a volume of 2.33 L?
PV=nRT? chemistry, ideal gas equation help?
firstly lemme tell u its a combination of th followin 3: 1.boyle's law- V proportional 1/P [P is pressure] 2.charles's law- V proportional to T [T is temperature] 3.avogadro's law- V proportional to n [n is number of moles/amount of gas] and V is the volume of gas these 3 gives us the ideal equation;) =>V proportional to nT/P =>removing the proportionality gives us the constant R =>V= RnT/P therefore PV=nRT its kinda long sry..juz so that u dont forget it:) [R is the gas constant] however at STP(standard temp and pressure), pressure is aat 1 bar and temp is at 273K R = 0.082057 L atm/mol/K R can also b 8.3145 J/mol/K
When should I use the ideal gas law equation vs the combined gas law equation?
The Ideal Gas Law is used when you have one gas (or gas mixture) and a set temperature and pressure. PV=nRTThe combined gas law is actually the Ideal Gas Law written for one gas (or gas mixture) and two sets of temperature and pressure:P1V1=nRT1P2V2=nRT2 (the number of moles in each equation is the same)Dividing the first equation by the second equation, the number of moles and the Universal Gas Constant, R, cancel out and you getP1V1/(P2V2) = T1/T2 Combined Gas LawThis equation can be solved for any of the variables, given values for the others. Remember, temperature is always in Kelvin in gas problems.
Need help with Ideal Gas Law question?
PV = nRT *n = number of moles *R = universal gas constant (8.3145 J/mol K) Convert Temp(Celsius) into Kelvin = add 273 Convert Vol (mL) into L = 0.750 Solve for the CO2's number of moles: Molar mass of C = 12 g/mol Molar mass of O = 16 g/mol .: Molar mass of CO2 = 44 g/mol (44g/mol CO2)(1.25g CO2) = 35.2 mol Solve for P: = (nRT)/V = [(35.2 mol)(8.3145 J/mol K)(22.5 C + 273)]/ 0.750 L] = [ 35.2 mol * 8.3145 J/mol K * 295.5 K ] / 0.750 L (mol and K will cancel out) = 115 312.14 J per L
Is the ideal gas equation applicable for all fluids (gas or liquid)?
The behavior of real gases usually agrees with the predictions of the ideal gas equation to within + -5% at normal temperatures and pressures.At low temperatures or high pressures, real gases deviate significantly from ideal gas behavior.In 1873, while searching for a way to link the behavior of liquids and gases, the Dutch physicist Johannes van der Waalsrealized that two of the assumptions of the kinetic molecular theory were questionable.The kinetic theory assumes that gas particles occupy a negligible fraction of the total volume of the gas.It also assumes that the force of attraction between gas molecules is zero.Van der Waals proposed that we correct for the fact that the volume of a real gas is too large at high pressures by subtracting a term from the volume of the real gas before we substitute it into the ideal gas equation. He therefore introduced a constantconstant (b) into the ideal gas equation that was equal to the volume actually occupied by a mole of gas particles. Because the volume of the gas particles depends on the number of moles of gas in the container, the term that is subtracted from the real volume of the gas is equal to the number of moles of gas times b.P(V - nb) = nRTWhen the pressure is relatively small, and the volume is reasonably large, the nb term is too small to make any difference in the calculation. But at high pressures, when the volume of the gas is small, the nb term corrects for the fact that the volume of a real gas is larger than expected from the ideal gas equation.To correct for the fact that the pressure of a real gas is smaller than expected from the ideal gas equation, van der Waals added a term to the pressure in this equation. This term contained a second constant (a) and has the form: an2/V2. The complete van der Waals equation is therefore written as follows.This equation is something of a mixed blessing.It provides a much better fit with the behavior of a real gas than the ideal gas equation.But it does this at the cost of a loss in generality. The ideal gas equation is equally valid for any gas, whereas the van der Waals equation contains a pair of constants (a and b) that change from gas to gas.see details inDeviations from the Ideal Gas Law