Question

Question 1: a. What is the accepted value of R in units of L x atm/mol...

Question 1:

a. What is the accepted value of R in units of L x atm/mol x K?

b. in units of L x torr/mol x K?

Homework Answers

Answer #1

a) Accepted value of R in units of L x atm/mol x K = 0.082057338   L atm K−1 mol−1

b) Accepted value of R in units of L x torr/mol x K = 62.363577    L Torr K−1 mol−1

The gas constant (also known as the molar, universal, or ideal gas constant, denoted by the symbol R or R) is a physical constant which is featured in many fundamental equations in the physical sciences, such as the ideal gas law and the Nernst equation.

It is equivalent to the Boltzmann constant, but expressed in units of energy (i.e. the pressure-volume product) per temperature increment per mole (rather than energy per temperature increment per particle). The constant is also a combination of the constants from Boyle's law, Charles's law, Avogadro's law, and Gay-Lussac's law.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1. A sample of gas occupies 5.27 L at a pressure of 2.63 atm. Determine the...
1. A sample of gas occupies 5.27 L at a pressure of 2.63 atm. Determine the new pressure (in atm) of the sample when the volume changes to 4.56 L at constant temperature. 2. Determine the temperature (in °C) of a 4.77-mol sample of CO2 gas at 6.11 atm in a container with a volume of 47.2 L. 3. Convert the pressure measurement of 2395 mmHg into units of atmospheres. 4. A latex balloon has a volume of 87.0 L...
A handbook lists the value of the Henry's Law constant as 1.400 ✕ 10−3 mol L-1...
A handbook lists the value of the Henry's Law constant as 1.400 ✕ 10−3 mol L-1 atm-1 for methane, CH4, dissolved in water at 25°C. Calculate the mole fraction of methane in water at an methane partial pressure of 380. torr.
Consider 1.00 mol of an ideal gas (CV = 3/2 R) occupying 22.4 L that undergoes...
Consider 1.00 mol of an ideal gas (CV = 3/2 R) occupying 22.4 L that undergoes an isochoric (constant volume) temperature increase from 298 K to 342 K. Calculate ∆p, q , w, ∆U, and ∆H for the change. For Units, pressure in atm and the rest in J.
The following table provides some information on carbon dioxide solubility in water. C (mol/L) P (atm)...
The following table provides some information on carbon dioxide solubility in water. C (mol/L) P (atm) k (mol/L⋅atm) T (∘C) 3.80×10−2 1.00 20.0 4.90×10−2 20.0 1.00 3.40×10−2 25.0 At 1 atm, how many moles of CO2 are released by raising the temperature of 1 liter of water from 20∘C to 25∘C?
1) At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an...
1) At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 45 ∘C ? Express your answer with the appropriate units. 2) One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 304...
calculate the pressure if nitrogen triflouride in atmospheres if 271.7 g are present in 60.0 L...
calculate the pressure if nitrogen triflouride in atmospheres if 271.7 g are present in 60.0 L vessel at a tenperature if 48 C (R=0.08206 L x atm x mol^-1 x K^-1) answer atm( number only what is the chemical formula for trifluoride?
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g)...
Calculate ΔG∘ (in kJ/mol) for the following reaction at 1 atm and 25 °C: C2H6 (g) + O2 (g)  → CO2 (g) + H2O (l) (unbalanced) ΔHf C2H6 (g) = -84.7 kJ/mol; S C2H6 (g) = 229.5 J/K⋅mol; ΔHf ∘ CO2 (g) = -393.5 kJ/mol; S CO2 (g) = 213.6 J/K⋅mol; ΔHf H2O (l) = -285.8 kJ/mol; SH2O (l) = 69.9 J/K⋅mol; SO2 (g) = 205.0 J/K⋅mol
In water at 68°F at sea level (1 atm), water contains about 42 mg/L of dissolved...
In water at 68°F at sea level (1 atm), water contains about 42 mg/L of dissolved oxygen. Determine the value of Henry's law constant for oxygen dissolving in water. Recall that air is 21% oxygen. A) 6.3 ´ 10–3 mol/(L atm) B) 0.010 mol/(L atm) C) 0.25 mol/(L atm) D) 1.9 ´ 10–2 mol/(L atm) E) 1.3 ´ 10–3 mol/(L atm)
A 10 mL of 120 mg/L solution of Styrene in water is injected into a 125...
A 10 mL of 120 mg/L solution of Styrene in water is injected into a 125 mL vial at 20°C. What will be the gas phase concentration at equilibrium? The Henry's Constant for Styrene is KH= 2.60 atm•L/mol The molar mass of Styrene is 104 g/mol Other Info: R= 0.08206 atm•L/mole•K = 1.987 cal/mole•K = 8.314 J/mole•K 1 Joule = Newton • Meter 1 atm = 1.013 X 105 N/m2 = 1.013 X 105 Pa 1 gallon = 3.785 L
Part A Initially, only A and B are present, each at 2.00 mol L−1. What is...
Part A Initially, only A and B are present, each at 2.00 mol L−1. What is the final concentration of A once equilibrium is reached? Express your answer to two significant figures and include the appropriate units. The reversible chemical reaction A(aq)+B(aq)⇌C(aq)+D(aq) Part B What is the final concentration of Dat equilibrium if the initial concentrations are [A] = 1.00 mol L−1 and [B] = 2.00 mol L−1 ? Express your answer to two significant figures and include the appropriate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT