Water Vapor Pressure TableGases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas,the vapor pressure of the water at that temperature must be subtracted from the total pressure.1) Consider the following reaction:Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)The total pressure of gas collected over water is 650.0 mmHg and the temperature is 23.0°C What is the pressure of hydrogengas formed in mmHg?Pressure 628.9mmHg KGAS LAW IDEAL GAS LAW CONSTANTINTRODUCTIONLABORATORY SIMULATION♦A Lab DataMass of magnesium (g)Moles of magnesium (mol)Temperature of water (°C)Temperature of water (K)Vapor pressure of water (mmHg)Barometric pressure (mmHg)ObservationsbubblyVolume of hydrogen gas collected (mL)Volume of hydrogen gas collected (L)Pressure of hydrogen gas (mmHg)Pressure of hydrogen gas (atm)Moles of hydrogen gas produced (mol)Ideal gas constant (L-atm-mol¹ K¹)How to calculate ideal gas constant0.2120.19824.0297.1524.01130-XWater Vapor Pressure TableES

Dalton's Law of partial pressures states that the total pressure exerted by a mixture of…

Water Vapor Pressure Table Gases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂(g) The total pressure of gas collected over water is 650.0 mmHg and the temperature is 23.0°C What is the pressure of hydrogen gas formed in mmHg? Pressure 628.9 mmHg

Water Vapor Pressure Table Gases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂(g) The total pressure of gas collected over water is 650.0 mmHg and the temperature is 23.0°C What is the pressure of hydrogen gas formed in mmHg? Pressure 628.9 mmHg

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the amount of salt in a commercial cold-pack containing ammonium nitrate (ΔHsol = + 25.7 kJ/mol) if the final temperature of the cold-pack is 3ºC. Assume that the initial temperature of water is 25ºC, mass of solution is 25 g and the specific heat of the solution is 4.184 J/g.K.
2. Suppose you performed a similar experiment using an unknown sample of carbonate. The pressure and volume were measured after the temperature stabilized at 21.5 °C. Given the data in the table below, what is the stoichiometric ratio between HCl(aq) and CO2(g)? Metal carbonate + HCl(aq) = Metal chloride + CO2(g) + H2O(1) Initial pressure (atm) 1.0 Initial gas volume (mL) 240.0 Volume of 1.0 M HCl solution added to fully consume the carbonate sample (mL) 22.0 Final pressure (atm) 2.32 Final gas volume (mL) 218.0
Ethylene (C2H4) plays an important role in the ripening of certain fruits and vegetables. It is sometimes supplemented under controlled conditions at produce—processing facilities but is also produced naturally by many fruit-bearing plants. Although the actual process by which plants produce ethylene is a complex one, imagine that it is produced by the simple breakdown of glucose according to the equation: C6H12O6 (s) à 3 C2H4 (g) + 3 O2 (g) Given S°= 212.1 J/molK, DG°= -910.56 kJ/mol and DH°= -1274.5 kJ/mol for C6H12O6 (s). a.) Determine the sign of DS° for the reaction. b.) Calculate DS° for the reaction. c.) Using the tabulated DG° values in the appendix, calculate DG° for the reaction. d.) Above what temperature (in °C) is the reaction spontaneous? Hint: you will first have to calculate DH° using tabulated values.
5.21 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
Which of the following statements is a true statement concerning a reaction that has reached a state of equilibrium? A system has reached equilibrium when the concentrations of reactants and products remain constant. A system has reached equilibrium when the reaction has stopped and no more products are formed. A system has reached equilibrium when the rate constant for the forward reaction equals the rate constant of the reverse reaction. A system has reached equilibrium when the concentrations of reactants and products correspond to the stoichiometric ratios determined by the balanced equation.
3.56 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･ °C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
3.76 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70 °C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g °C and the density of the water is 1.00 g/ mL). You can assume that the specific heat of the solution is the same as that of water.
What is the enthalpy of reaction, ΔHrxn for the reaction of nitrogen gas with oxygen gas to produce NO2(g), based on the following information? These reactions are not at standard state or at 298 K. N2(g) + O2(g) → 2 NO(g); ΔH = 332.9 kJ2 NO2(g) → 2 NO(g) + O2(g); ΔH = 718.4 kJ Report your answer in kJ to 1 decimal place.
Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (M9SO,·7H,O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 73.25 g. What is the mass in grams of the original salt mixture that you must add to 1.000L of water to make a 0.1000 M solution of Mg2+ ion?
4.71 g of MgSO4 is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate AH, in kJ/mol, for the dissolution of MgSO4. (The specific heat of water is 4.184 J/g.°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
4.06 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.18 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.
5.61 g of MgSO₄ is placed into 100.0 mL of water. The water's temperature increases by 6.70°C. Calculate ∆H, in kJ/mol, for the dissolution of MgSO₄. (The specific heat of water is 4.184 J/g･°C and the density of the water is 1.00 g/mL). You can assume that the specific heat of the solution is the same as that of water.