A 11.0 L tank contains 0.234 kg of helium at 20.0 ∘C. The molar mass of helium is 4.00 g/mol .
A) How many moles of helium are in the tank?
B) What is the pressure in the tank, in pascals?
C) What is the pressure in the tank, in atmospheres?
A 11.0 L tank contains 0.234 kg of helium at 20.0 ∘C. The molar mass of...
A 20.6-L tank contains 0.206 kg of helium at 16.4°C. The molar mass of helium is 4.00 g/mol. (a) How many moles of helium are in the tank? mol (b) What is the pressure in the tank, in pascals and in atmospheres? Pa ? atm?
A 11.0 L tank contains 0.280 kg of helium at 18.0°C. The molar mass of helium is 4.00 g/mol Part B What is the pressure in the tank, in pascals? Express your answer in pascals. IVO AXO ao ? Submit Request Answer Part What is the pressure in the tank, in atmospheres? Express your answer in atmospheres. VO Alicbm O ? p= 197 atm Submit Previous Answers Request Answer X Incorrect; Try Again: 4 attempts remaining
A 12.0 L tank contains 0.305 kg of helium at 16.0 ∘C. The molar mass of helium is 4.00g/mol. 1)How many moles of helium are in the tank? 2)What is the pressure in the tank (in pascals)? 3) What is the pressure in the tank ( in atm)?
both please How many moles of helium are in the tank? Express your answer using three significant figures. Constants A 12.0 L tank contains 4.46x104 kg of helium at 19.0 °C. The molar mass of helium is 4.00 g/mol. You may want to review (Pages 585-590) For related problemsolving tips and strategies, you may want to view a Video Tutor Solution of Volume n-61.25 mol SubmitP Previous Answers Reguest Ans X Incorrect, Try Again; 8 attempts remaining: no points deducted...
A tank contains 22.0 grams of oxygen, 80.00 grams of helium, and 3.21 moles of hydrogen gases.The mixture has a total pressure of 7.00 atmospheres. Calculate the following. a) How many moles of O2 are in the tank? b) How many moles of He are in the tank? c) Total moles of gas in tank d) Mole fraction of each gas e) The partial pressures of each gas
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?
Helium gas with a volume of 3.50 L , under a pressure of 0.190 atm and at a temperature of 45.0 ∘C, is warmed until both pressure and volume are doubled.What is the final temperature?How many grams of helium are there? The molar mass of helium is 4.00 g/mol.
A steel tank contains 232 g of ammonia gs (NH3 with molar mass 17.0 g/mol) at a pressure of 1.45 x 106 and a temperature of 45.4oC. (a) What is the volume of the tank in liters? (b) Later the temperature is 42.0oC and the pressure is 0.967 x 106 Pa. How many grams of gas have leaked out of the tank? (Ignore the thermal contraction of the tank.)
A 21.8-L tank of carbon dioxide (CO22) is at a pressure of 9.28 atm and temperature of 19.4∘∘C. (a)Calculate the number of moles of gas in the tank. ______________ mol ( ± 0.02 mol) (b)Obtain the number of grams of carbon dioxide in the tank. Hint: You can obtain the molar mass of CO22 by adding the molar mass of C and twice the molar mass of O. The molar mass of an element is given on the periodic table...
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