Use the following information to identify the diatomic molecule A and the compound B, then answer the following questions.
An empty glass container has a mass of 658.572 g. It has the mass of 659.452 g after it has been filled with nitrogen gas at a pressure of 790. torr and a temperature of 15.0 degrees C. When the container is evacuated and refilled with the diatomic molecule A at a pressure of 745 torr and a tempurature of 26.0 deg C, it has a mass of 660.590 g.
Compound B is a gaseous organic compound that consists of 85.6% carbon and 14.4% hydrogen by mass. Exactly 18.384 g of the compound is placed in a stainless steel vessle (10.68 L) with 4.63 mol of oxygen gas at 22.0 deg C. The total pressure in the vessel is 11.98 atm.
a) What is the diatomic molecule A?
b) What is compound B?
c) A and B react quantitatively in a 1:1 molar ratio to form one mole of the single product, gas X. Write a balanced equation to determine the molecular formula of gas X.
d) How many grams of gas X will be produced if 10.0 L or A and 8.60 L of B (each at STP) are reacted by opening a stopcock connecting the two samples?
e) What will be the total pressure in the sysem?