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?
To answer the questions, let's break down the given information step by step:
(1.) Identify M, B, D, and X. Write a balanced equation for the reaction between M and HX.
- From the question, we know that M is a solid element that reacts with HX to form compound C and gas D.
- B is the monoprotic acid, which is represented by HX.
- D is the gas that is produced during the reaction.
- X is the halogen element that is part of the compound C.
To write a balanced equation between M and HX, let's first determine the chemical formula of compound C. We know that compound C is a binary salt containing elements M and X.
Since M reacts with the hydrogen halide HX, we can assume that the compound C will be an ionic compound. Therefore, the formula of compound C will be MX, where X represents the halogen element.
The balanced equation for the reaction between M and HX is:
M + HX -> MX + D
(2.) What mass of compound C will be formed, and what molar concentration will it have in the final mixture? Assume that the volume of the final mixture is 50.00 ml.
To calculate the mass of compound C formed, we need to know the molar mass of M and the stoichiometric ratio between M and compound C. Unfortunately, the molar mass of M is not provided in the given information, so we cannot determine the mass of compound C.
However, we can calculate the molar concentration of compound C in the final mixture. Since the volume of the final mixture is given as 50.00 ml, the molar concentration of compound C can be calculated using the formula:
Molarity (M) = moles of solute / volume of solution (in liters)
Given that the volume of the solution is 50.00 ml (or 0.0500 L) and assuming the reaction goes to completion with 100% yield, the moles of compound C can be calculated by the stoichiometric ratio:
1 mole of M reacts to form 1 mole of compound C.
Therefore, the molar concentration of compound C in the final mixture will be:
Molarity of C = Moles of C / Volume of solution
Since the moles of C will be equal to the moles of M used in the reaction (assuming 100% yield), we need to calculate the moles of M used.
Moles of M used = Mass of M used / Molar mass of M
(3.) Gas D is collected by water displacement at 23 degree C and an atmospheric pressure of 755 torr. What volume should be collected?
To calculate the volume of gas D collected, we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = moles of gas
R = Ideal gas constant
T = Temperature (in Kelvin)
In this case, we are given the pressure in torr. To convert it to atm, we divide by 760 (since 760 torr = 1 atm):
Pressure (in atm) = 755 torr / 760 torr/atm = 0.9934 atm
The temperature is given as 23 degrees Celsius. To convert it to Kelvin, we add 273.15:
Temperature (in Kelvin) = 23 + 273.15 = 296.15 K
We need to calculate the moles of gas D to determine the volume. Since we are given the mass of element D (3.000g) and the molar mass of D is not provided, we cannot directly calculate the moles of D. Therefore, we cannot determine the volume of gas D collected.
(4.) How many moles of which reactant are left over when the reaction is completed?
To determine the moles of reactant left over when the reaction is completed, we need to compare the stoichiometric ratio between the reactants.
Let's consider the reaction between M and HX:
M + HX -> MX + D
From the balanced equation, we can see that 1 mole of M reacts with 1 mole of HX to form 1 mole of MX and 1 mole of D.
Given that the student places 1.05g of M in the reaction, we can calculate the moles of M used:
Moles of M used = Mass of M used / Molar mass of M
Once we have the moles of M used, we can also determine the moles of HX used since the stoichiometric ratio is 1:1.
Finally, to calculate the moles of each reactant left over, we need to subtract the moles used from the initial moles of each reactant.
Please provide the molar mass of M to proceed with the calculations.