posted by Patrick .
Element M(a solid) reacts with an aqueous solution of compound B to form an aqueous solution of compound C(a salt) and a gas composed of element D. When 1.000g of element M is reacted with excess oxgen 1.658g of the compound MO are formed. Compound B is binary, monoprotic acid (hydrogen halide) HX. A student dissolves 1.000g of HX in enough water to make 50.00ml of solution and titrates it with 0.5000 M KOH. This requires 54.79ml of base to reach end point. Compound C is binary salt that contains elements M and X. A 3.000g sample of element D at STP occupies a volume of 33.3L. A student places 1.05g of M in 50.00ml of 1.00M HX. Assume the reaction goes to completion with 100% yield. (1.) Identify M, B, D, and X. Write a balanced equation for the reaction between M and HX.(2.) What mass of compound C will be formed, and what molar concentration will it have in the final mixature. ( Assume that the volume of the final mixture is 50.00 ml). (3.)Gas D is collected by water displacement at 23 degree C and an atmospheric pressure of 755torr. What volume should be collected? (4.) How many moles of which reactant are left over when the reaction is completed?
This is called a "railroad" problem. We called them that in school when I was a student because they were designed to "railroad" us out of class.:-).
It's long, it a lot of work, and I shall be more than happy to help you through it BUT surely you must know SOMETHING about it. Where are you stumped? And it would help if you reposted at the top of the page along with your thoughts about how to proceed.