Use the following information to identify element A and compound B, then answer questions a and b.
I'm so stuck on this problem and don't know where to begin. I need to have this problem done by Wednesday. PLEASE HELP!!!
An empty glass container has a mass of 658.572 g. It has a mass of 659.452 g after it has been filled with nitrogen gas at a pressure of 790. torr and a temperature of 15⁰C. When the container is evacuated and refilled with a certain element (A) at a pressure of 745 torr and a temperature of 26⁰C, it has a mass of 660.59 g.
Compound B, a gaseous organic compound that consists of 85.6% carbon and 14.4% hydrogen by mass, is placed in a stainless steel vessel (10.68L) with excess oxygen gas. The vessel is placed in a constant-temperature bath at 22⁰C. The pressure in the vessel is 11.98 atm. In the bottom of the vessel is a container that is packed with Ascarite and a dessicant. Ascarite is asbestos impregnated with sodium hydroxide; it quantitatively absorbs carbon dioxide:
2NaOH (s) + CO2 (g) „³ Na2CO3 (s) + H2O (l)
The dessicant is anhydrous magnesium perchlorate, which quantitatively absorbes the water produced by the combustion reaction as well as the water produced by the above reaction. Neither the Ascarite nor the desiccant reacts with the compound B or oxygen. The total mass of the container with the Ascarite and desiccant is 765.3 g.
The combustion reaction of compound B is initiated by a spark. The pressure immediately rises, then begins to decrease, and finally reaches a steady value of 6.02 atm. The stainless stell vessel is carefully opened, and the mass of the container inside the vessel is found to be 846.7 g.
A and B react quantitatively in a 1:1 mole ratio to form one mole of the single product, gas C.
a. How many grams of C will be produced if 10.0L of A and 8.60: of B (each at STP) are reacted by opening a stopcock connecting the two samples?
b. What will be the total pressure in the system?
14 answers
Next you want to determine the empirical formula of gas B.
What do you do next?
The container is filled with gas B and oxygen to a combined total pressure of 11.98 atm (pressure gas B + pressure oxygen = 11.98 atm). The mixture is combusted, the pressure settles to 6.02 atm, MEANING that 11.98 atm - 6.02 atm = mols B + oxygen used. I would substitute that pressure in PV = nRT and determine the number of mols used up in the combustion.
1. How many mols gas B + oxygen were used in the combustion of gas B?2. How many grams of CO2 and H2O were formed in the combustion of gas B?