If 3.95 kg of propane gas (C3H8) is stored in a 68.5 L container at 19.1°C,...
If 5.49 kg of propane gas (C3H8) is stored in a 86.8 L container at 15.9oC, what pressure (in atm) will be exerted on the storage tank? Give your answer to the correct number of significant figures and in units of atm. Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1, Molar mass (g/mol) of C = 12.01 H = 1.008.
A 1.75 L volume of helium gas stored at 0.873 atm will have a temperature of 46.9oC. If the helium is compressed down to a volume of 523 mL while allowing the pressure to settle at 1,662 mmHg, what will the temperature of the helium gas now be, in oC? Give your answer to one decimal place, and in units of oC. Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1.
A 2.337 g sample of magnesium carbonate (MgCO3) was dissolved in hydrochloric acid. The following reaction occurred at 27.1oC and a pressure of 784 mmHg: MgCO3(s) + 2HCl(aq) --> CO2(g) + H2O(l) + MgCl2(aq) Calculate the volume (in mL) of CO2 produced. Give your answer to the correct number of significant figures and in units of mL. Data: 1 atm = 760 mmHg, 0oC = 273 K, PV = nRT, R = 0.0821 L.atm.mol-1.K-1, Molar mass (g/mol) of Mg =...
A 45.0-L steel tank at 20.0°C contains acetylene gas, C2H2, at a pressure of 1.39 atm. Assuming ideal behavior, how many moles of acetylene are in the tank? De Formulas you MAY need. PV=nRT R -0.0821 atm.L/mol.K K - T°C + 273 latm - 760 mmHg
A 75.0 L steel tank at 20.0 degrees C contains propane gas, C3H8, at a pressure of 1.39 atm. Assuming ideal behavior, how many moles of C atoms are in the tank?
A 125 mL glass bulb contains 0.138 g sample of propane, C3H8, at 22C. What is the pressure of this gas? [R = 0.0821 L atm mol-1 K-1] a. 0.61 atm b. 0.28 atm c. 0.045 atm d. 0.0061 atm e. 0.000045 atm Acetylene can be made by reacting calcium carbide with water: CaC2(s) + 2 H2O(l)→Ca(OH)2(s) + C2H2(g) What is the maximum volume of acetylene that can be obtained from 225 g of calcium carbide at 23C and 645...
A gas occupies 240 mL at 283 K and 680 mmHg. What is the approximate final temperature would be required to increase the pressure to 1 atm while keeping the volume constant? (Hint-this is with initial conditions of V, T, and P and then the Final Temp is asked) PV = nRT R = 0.0821 L'atm/mol K 1 atm = 760 mmHg 43°C O 20°C O-95°C O 253°C O 316°C
The amount of gas that occupies 60.82 Lat 310 K and 367 mm Hg is mol. hint: use ideal gas law PV-nRT, and 1 atm - 760 mmHg, gas constant R-0.082, and OK --273°C 0.190 094 0.850 118 116
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 of 20 ned t Introduction to the Ideal Gas Law Part B A 200 L gas cylinder is iled with 8.00 moles of gas. The tank is stored at 27C What is the pressure in the tank? Learning Goal: To apply the ideal gas law to problems inwolving temperature, pressure, volume, and moles of a gas Express your answer to three significant figures and include the appropriate u Hints The lour properties of gases (pressure P. volume V temperature...