If the concentration of a gas in solution is 5.9 and the pressure exerted over the...
Calculate the pressure exerted by 10.5 moles of neon gas in a volume of 5.65 L at 25 ° C using (a) the ideal gas equation and (b) the van der Waals equation. (For neon, a = 0.211 atm · L2/mol2 and b = 0.0171 L/mol.) (a) atm (b) atm
What is the volume occupied by 1.000 mol of nitrogen gas at a pressure of 2.00 atm and a temperature of 100 K? Gas constant R = 0.08206 L.atm. mol.
9. Calculate the pressure exerted by 5.00 mol of Co2 in a 1.00 L vessel at 300 K (a) assuming the gas behaves ideally and (b) using the van der Waals equation. (a= 3.610 L'atm/mol, and b = 0.0429 L/mol).
will be exene 16. Gases are sold in large cylinders for laboratory use. What pressure, in atmospheres, will be ex by 2500 g of oxygen gas (O2) when stored at 22°C in a 40.0 L cylinder (R=0.08206 L'atm-K--moll)? A) 3.55 atm B) 1510 atm C) 47.3 atm D) 7.56 x 104 atm E) 10.2 atm 17. Assuming ideal behavior, what is the density of argon gas at STP (standard Temperature and Pressure), in g/L (R = 0.08206 L'atm-K--moll)? [Formula: d...
Be sure to answer all parts. Calculate the pressure exerted by 2.65 moles of CO2 confined in a volume of 4.03 L at 456 K. What pressure is predicted by the ideal gas equation? The van der Waals constants for CQ area 3.59 atm. L2/mol2 and b 0.0427 L/mol. van der Waals equation: ideal gas equation: [24.6 ]atm
Suppose you have a fixed container containing 0.255 moles of a gas (the identity of the gas doesn't matter). If the container volume is 0.748 L, and the temperature is 301.15 K, what is the pressure in atm? (R=0.0821 L'atm/mol-K) O A.0.784 atm OB. 0.00842 atm O C.7.84 x 104 atm D.8.42 atm
Please i need help to solve these problem Chem. If an ideal gas has a pressure of 2.13 atm, a temperature of 309 K, and has a volume of 59.73 L, how many moles of gas are in the sample A 6.8 increased its volume to 34.4 L. What was the initial volume of the balloon? s mol sample of freon gas was placed in a balloon. Adding 3.50 mol of freon gas to the balloon A hot air balloon...
Calculate the concentration of CO2 in water at 25°C when the pressure of CO2 over the solution is 6.1 atm. At 25°C, the Henry's law constant for CO2 in water is 3.1 × 10−2 mol/L · atm.
Calculate the pressure exerted by 18.0 g of N2 in a 700. mL vessel at 298 K using the ideal gas equation. Then, recalculate the pressure using the van der Waals equation. Assuming that the pressure calculated from the van der Waals equation is correct, what is the percent error in the answer when using the ideal gas equation? Van der Waals constants for N2 are: a= 1.39 atm*L^2/mol^2 , and b=0.0391 L/mol ; R=0.082057 L*atm/K*mol. Pideal gas law =...
1. A constant amount of gas occupies 16.2 L at 313 K. What volume would that gas occupy at 336 K? 2. What’s the molarity of a solution containing 48.5 g of MgCl2 (Molar mass = 95.21 g/mol) in 1.75 L volume? 3. 7.215 moles of a gas occupies 105.1 L at a constant pressure. How many moles of that gas could occupy 175.6 L? 4.What volume of a 0.85 M stock solution would be needed to prepare 4.5 L...