Derive a gas law formula for a specific scenario One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 311 K, but the container does not expand. What will the new pressure be? Part A The most appropriate formula for solving this problem includes only which variables? Enter the required variables, separated by commas (e.g., P,V, T). > View Available Hint(s)

Consider the following balanced chemical equation. 5 F2 (g)  +  Br2 (l)    →   2 BrF5 (l) 0.789 atm of F2 in a 0.1250 L container at 26.5 °C reacted. How many mol of BrF5 were formed? SHOW WORK. Write out the problem on paper showing all conversion factors, unit cancellations, calculations, s.f., etc. Answer the questions related to the setup and calculation for this problem. Be sure to use our periodic table to calculate any molar masses needed (rounded to proper number of decimal places), otherwise your values might be slightly off and answers may be marked as incorrect. Abbreviate units as follows: grams = g, moles = mol, liters = L, atmospheres = atm   What temperature (with proper s.f.) is entered into the equation? Enter the value in the first blank and the units in the second blank.     Calculate the mol of F2 reacted (enter value only, with proper s.f.).  mol   Use the three blanks to enter the number, unit, and substance (in this order) that appears in the denominator of the…

The ideal gas law is a limiting law, in that it is expected to hold as pressure approaches zero. Suppose the following measured values have been obtained for oxygen gas at 273.15K. Based on the data, calculate R for each pressure value and create a table of pressure and R values (i.e. you are treating R as a variable rather than a constant at this point). Then create a plot R vs p and find the “best value” of R by determining the y-intercept of a straight line fit. (Be sure to label your axes including units).

A flask contains a mixture of two gases: NO2 and Ne. The flask holds 0.519 mol of NO2 and an unknown amount of Ne. If the partial pressure of Ne is 0.43 bar and the total pressure in the flask is 0.83 bar, calculate the mass of Ne in the flask (in g). TIP: You don't need the volume of the flask nor the temperature to solve this problem. Express answer in 2 significant figures.