PHYSICAL CHEMISTRY-STUDENT SOLN.MAN.
2nd Edition
ISBN: 9781285074788
Author: Ball
Publisher: CENGAGE L
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Chapter 4, Problem 4.29E
Analogous to equation 4.26, what is the expression for
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Aqueous hydrochloric acid reacts with solid calcium metal to form a solution of calcium chloride and hydrogen gas. The reaction is highly spontaneous and proceeds to completion. A chemist reacts 65.30 g calcium with excess hydrochloric acid at STP. You may assume the gas behaves ideally under all conditions.
(a) What volume of hydrogen gas is produced over water?
(b) What is the final concentration (in mol/L) of calcium chloride in the solution if the initial acid solution had a volume of 0.85 L? Assume no change in solution volume.
(c) All of the hydrogen gas that evolved during the reaction is collected and held in a rigid flask with a volume of 11.40 L. If the pressure in the flask cannot exceed 3.60 atm, what is the maximum temperature at which the gas can be stored in the flask?
Dalton's law states that in a mixture of chemically non-interacting gases, thethe pressure exerted by each contributor at a certain temperature is the same as if it were alone in thein the container alone, and that the total pressure is equal to the sum of the partial pressures(1) of each gas. Deduce this law by kinetic theory from equation 18.11.
(1)The partial pressure of a gas in a mixture of ideal gases corresponds to the pressure it would exert if it werealone, occupying the whole container, at the same temperature of the ideal mixture.
P = F/A = N*m*Vx^2/V (18.11)
Define the concept of Ideal Gad & also discuss the Multiplicity of a Monatomic Ideal Gas ?
Chapter 4 Solutions
PHYSICAL CHEMISTRY-STUDENT SOLN.MAN.
Ch. 4 - List the sets of conditions that allow dS, dU, and...Ch. 4 - Explain why conditions for using S>0 as a strict...Ch. 4 - Explain how the equation dU+pdVTdS0 is consistent...Ch. 4 - Explain why the spontaneity conditions given in...Ch. 4 - Prove that the adiabatic free expansion of an...Ch. 4 - Derive equation 4.6 from equation 4.5.Ch. 4 - Derive equation 4.8 from equation 4.7.Ch. 4 - The third part of equation 4.9 mentions a...Ch. 4 - Calculate A for a process in which 0.160mole of an...Ch. 4 - What is the maximum amount of non-pV work that can...
Ch. 4 - Consider a piston whose compression ratio is 10:1;...Ch. 4 - When one dives, water pressure increases by 1atm...Ch. 4 - Calculate G(25C) for this chemical reaction, which...Ch. 4 - Thermodynamic properties can also be determined...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - For the reaction C(graphite)C(diamond) at 25C,...Ch. 4 - Determine G for the following reaction at 0C and...Ch. 4 - What is the maximum amount of electrical that is,...Ch. 4 - When a person performs work, it is non-pV work....Ch. 4 - Can non-pV work be obtained from a process for...Ch. 4 - Can pV work be obtained from a process for which...Ch. 4 - Batteries are chemical systems that can be used to...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - Under what conditions is A=0 for a phase change?...Ch. 4 - Example 4.2 calculated A for one step of a Carnot...Ch. 4 - Can CV and Cp be easily defined using the natural...Ch. 4 - Analogous to equation 4.26, what is the expression...Ch. 4 - Prob. 4.30ECh. 4 - Prob. 4.31ECh. 4 - Prob. 4.32ECh. 4 - Although ideally, U=H=0 for a gas-phase process at...Ch. 4 - Use equations 4.21 and 4.25 to explain why H and G...Ch. 4 - Prob. 4.35ECh. 4 - Which of the following functions are exact...Ch. 4 - Prob. 4.37ECh. 4 - Prob. 4.38ECh. 4 - Prob. 4.39ECh. 4 - Equation 4.19 says that (UV)S=p If we are...Ch. 4 - For an isentropic process, what is the approximate...Ch. 4 - Use the ideal gas law to demonstrate the cyclic...Ch. 4 - Prob. 4.43ECh. 4 - Prob. 4.44ECh. 4 - Evaluate (U/V)T for an ideal gas. Use the...Ch. 4 - Evaluate (U/V)T for a van der Waals gas. Use the...Ch. 4 - Repeat the previous exercise for a gas that...Ch. 4 - Determine an expression for (p/S)T for an ideal...Ch. 4 - Determine the value of the derivative {[(G)]/T}p...Ch. 4 - Prob. 4.50ECh. 4 - Prob. 4.51ECh. 4 - A 0.988-mole sample of argon expands from 25.0L to...Ch. 4 - A 3.66-mol sample of He contracts from 15.5L to...Ch. 4 - Prob. 4.54ECh. 4 - Prob. 4.55ECh. 4 - Use the Gibbs-Helmholtz equation to demonstrate...Ch. 4 - For the equation 2H2(g)+O2(g)2H2O(g)...Ch. 4 - Use equation 4.46 as an example and find an...Ch. 4 - What is the value of G when 1.00mol of water at...Ch. 4 - Prob. 4.60ECh. 4 - Prob. 4.61ECh. 4 - Prob. 4.62ECh. 4 - Prob. 4.63ECh. 4 - Prob. 4.64ECh. 4 - What is the change in the chemical potential of a...Ch. 4 - Prob. 4.66ECh. 4 - Prob. 4.67ECh. 4 - Prob. 4.68ECh. 4 - Prob. 4.69ECh. 4 - Can equation 4.62 be used to calculate for an...Ch. 4 - Prob. 4.71ECh. 4 - Of helium and oxygen gases, which one do you...Ch. 4 - Prob. 4.73ECh. 4 - Use equation 4.39 to determine a numerical value...Ch. 4 - Prob. 4.75ECh. 4 - Prob. 4.76E
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- Use the ideal gas law to symbolically prove the cyclic rule of partial derivatives.arrow_forwardUse the ideal gas law to demonstrate the cyclic rule of partial derivatives.arrow_forwardUse the data in Table 2.2 to determine PH T for N2 at 50C and 20atm. Make any reasonable assumptions necessary.arrow_forward
- What properties of a nonideal gas do the Vander Waals constants represent?arrow_forwardUnder what conditions of temperature does a Redlich-Kwong gas behave like an ideal gas? Use the Redlich-Kwong equation of state to justify your answer.arrow_forwardUse equation 4.46 as an example and find an expression for A as the volume varies.arrow_forward
- The ideal gas law is theequation of state for an ideal gas. Why cantit be used to determine TpH?arrow_forwardWhich of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_forwardCalculate the following quantities for an ideal gas: The pressure of the gas, if 0.0499 mole occupies 0.525 L at 100 °C.arrow_forward
- It is desired to market O2 in small cylinders having volumes of 15L and each containing 2 kg of O2. If the cylinders may be subjected to a maximum temperature of 500C, calculate the pressure, for which they may be designed, assume the applicability of the ideal gas law.arrow_forwardWhich on the following statements is false? In a mixture, each gas can not be considered ideal, therefore one can not use the ideal gas equation in order to determine the partial pressure of a particular gas. The molar volume is the same for all ideal gases at STP. The total pressure of a particular gas in a mixture of gases can be determined by multiplying the total pressure of the mixture by the mole fraction (# of moles of the gas in question divided by the total number of moles) of the gas in question. In general, amount of vapour pressure increases with a rise in temperature. In a mixture of gases, the total pressure is equal to the sum of the partial pressures of each gas in the mixture.arrow_forward2. The atmospheric temperature at altitudes where jetliners fly is approximately -33°C. Calculate the average and molar kinetic energies of molecular nitrogen (N2) at this temperature.arrow_forward
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