posted by Patrick on .
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?