A 5.0-liter gas tank holds 1.4 moles of helium (He) and 0.70 moles of 0 xygen (O2), at a temperature of 260 K. The atomic masses of Helium and oxygen are 4.0 g/mol and 16.0 g/mol, respectively. Questions from 7 to 9 are based on this information Question: The rms speed of Helium atom is closest to a. 450 m/s b. 1273 m/s c. 2500 m/s d. 840 m/s e. None of the above.
Consider the combustion of butane (C4H10) : 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l) In a particular reaction, 5.72 moles of C4H10 are reacted with an excess of O2. Calculate the number of moles of CO2 formed. Be sure your answer has the correct number of significant digits. molCO2 ×10
3.60 moles CO, 3.60 moles H2O, 1.00 moles CO2, and 1.00 moles H2 are put in a 2.00 L container at 600∘C. CO(g) + H2O(g) ⇄ CO2(g) + H2(g) Keq = 10.0 Calculate the equilibrium concentration of CO2. (4 marks)
For the following reaction, 0.156 moles of carbon disulfide are mixed with 0.187 moles of chlorine gas. carbon disulfide(s) + chlorine(g) → carbon tetrachloride(ℓ) + sulfur dichloride (s) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of carbon tetrachloride that can be produced? Amount = moles
How many moles are present in a 185. g sample of X(NO3)2. The molar mass of element X is 119.57 g/mol. Use the correct number of significant figures in your answer. Do not enter the unit.
To what final volume must 115.9 mL of 0.165 MH2 SO4 solution be diluted to give a 0.0500 MH2 SO4 solution? Vfinal = mL
The following reaction has an equilibrium constant K = 4.00×10−3. 2HCN(g) ⇌ H2(g) + C2N2(g) Some amounts of HCN and H2 are introduced into a reaction vessel, and the system is allowed to come to equilibrium. The resulting equilibrium concentrations are [HCN] = 0.970 M, and [C2N2] = 0.042 M. Calculate the equilibrium concentration of H2. Answer in molarity to at least three significant figures.
A 4.60 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.20 M, where it remained constant. A(s) ⇌ B(g) + C(g) Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain? moles of A : mol
When 6.000 moles of glucose are combusted, 16815 kJ of energy is produced. Which of the following chemical equations represent this process? 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = −2802.5 kJ 6C6H12O6(s) + 36O2(g) → 36CO2(g) + 36H2O(l) ΔH = 16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −16815 kJ C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l) ΔH = −2802.5 kJ all equations are correct
Calculate the total pressure in a binary system where the mole fraction of A in the vapor phase is 0.200, the vapor pressure of pure A is 100. mmHg and the vapor pressure of pure B is 300. mmHg. A) 80.0 mmHg B) 214 mmHg C) 140. mmHg D) 260. mmHg E) Cannot be determined
An analytical chemist is titrating 137.4 mL of a 0.2300 M solution of methylamine (CH3NH2) with a 0.1600 M solution of HNO3. The pKb of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 223.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.