Answer: molarity of HCI = 2. Calculate the volume in L) of 1.63 mol of CO2...
The volume of 3.3 mol of ideal gas is 45.7 L at 350 K. Calculate its pressure (in atmospheres). L atm L kPa • Use R = 0.08206 314 for the ideal gas constant. mol K Your answer should have two significant figures. Do NOT include units in your response. mol K for the Provide your answer below:
1a) Calculate the Volume in L of 1.2 moles of CH4 confined in a container at a pressure of 10 atm at 323 K. Use the ideal gas equation. C=12 g/mol H= 1 g /mol T(K)= T(°C)+273.15 R=0.0821 L-atm/mol-K PV=nRT answer a)0.318 b)90.2 c)3.18 d)31.8 1b) Is the number of particles or spheres in the cubic cell centered on the body? answer 1)3 2)4 3)1 4)2 3c) in the solid state does it form molecular crystals answer a)NaCL b)graphite c)CO2...
1. Calculate the volume of the gas, in liters, if 1.55 mol has a pressure of 1.20 atm at a temperature of -6 ∘C. (Answer in L) 2.Calculate the absolute temperature of the gas at which 3.33×10−3 mol occupies 498 mL at 760 torr . (Answer in K) 3.Calculate the pressure, in atmospheres, if 2.65×10−3 mol occupies 415 mL at 140 ∘C. (Answer in atm) 4.Calculate the quantity of gas, in moles, if 127 L at 60.0 ∘C has a...
Resources A sample of an ideal gas has a volume of 3.35 L at 11.60 °C and 1.40 atm. What is the volume of the gas at 22.40 °C and 0.988 atm? A sample of an ideal gas has a volume of 2.27 L at 282 K and 1.15 atm. Calculate the pressure when the volume is 1.29 Lane the temperature is 308 K MacBook Pro Tv u op 7v | B If 5.42 mol of NO, occupy 46.3 L,...
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
3.45 mol of CO2(g) is confined to a volume of 5.00L at 450.K. This results in high pressure and non-ideal gas behavior. Determine the pressure in units of atm. Per Table 5.4 in the textbook, a = 3.59 atm·L2/mol2 and b = 0.0427 L/mol.
2 ml 0.50 M Volume of Stock Solution (mL) Molarity of Stock Solution (mol/L) Volume of Diluted Solution (mL) Molarity of Diluted Solution (mol/L) 10 ml
2. A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L system. The following equilibrium is established at 500 K CO2(g) + H2(c) -> CO(S) + H2O(g) At equilibrium, Prao = 3.51 atm. A) Calculate the equilibrium partial pressures of CO2. Hz, and CO (6 points) and B) Calculate Kfor the reaction (4 points). Recall PV = nRT, with R = 0.0821 L-atm/mol-K. Hint: ICE chart not necessary. Notice...
Part A Calculate the volume of the gas, in liters, if 1.60 mol has a pressure of 1.20 atm at a temperature of -5 ∘C. Express the volume in liters to three significant digits. V V = nothing L SubmitRequest Answer Part B Calculate the absolute temperature of the gas at which 3.53×10−3 mol occupies 478 mL at 760 torr . Express the temperature in kelvins to three significant digits. T T = nothing K SubmitRequest Answer Part C Calculate...
1.) Use the ideal gas law to calculate the volume occupied by 0.500 mol of nitrogen gas at 1.60 atm pressure and at 27°C. R = 0.0821 L*atm/(K*mol). 0.694 L 7.10 L 7.70 L 7.89 L (separate question) 2.What will be the final gas temperature in kelvins?