Open Question
When a 118-mL flask is evacuated, it has a mass of 97.129 g. Upon filling it with 768 torr of helium gas at 35 °C, the mass increases to 97.171 g. Based on this information, can we determine if the helium gas was pure?
Ch.5 - Gases
Chapter 5, Problem 101
Consider the reaction: 2 NiO(s) → 2 Ni(s) + O2(g). If O2 is collected over water at 40.0 °C and a total pressure of 745 mmHg, what volume of gas is collected for the complete reaction of 24.78 g of NiO?
Verified step by step guidance1
Calculate the molar mass of NiO by adding the atomic masses of Ni and O.
Determine the number of moles of NiO by dividing the given mass (24.78 g) by the molar mass of NiO.
Use the stoichiometry of the balanced chemical equation to find the moles of O2 produced. According to the equation, 2 moles of NiO produce 1 mole of O2.
Use the ideal gas law, PV = nRT, to calculate the volume of O2. First, convert the temperature from Celsius to Kelvin by adding 273.15.
Adjust the total pressure to account for the vapor pressure of water at 40.0 °C, then use the adjusted pressure in the ideal gas law to find the volume of O2.
Related Practice
Textbook Question
A gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 82.66% carbon and 17.34% hydrogen by mass. The mass of 158 mL of the gas, measured at 556 mmHg and 25 °C, was 0.275 g. What is the molecular formula of the compound?
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Textbook Question
A gaseous hydrogen- and carbon-containing compound is decomposed and found to contain 85.63% C and 14.37% H by mass. The mass of 258 mL of the gas, measured at STP, was 0.646 g. What is the molecular formula of the compound?
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Textbook Question
Consider the reaction: 2 Ag2O(s) → 4 Ag(s) + O2(g) If this reaction produces 15.8 g of Ag(s), what total volume of gas can be collected over water at a temperature of 25 °C and a total pressure of 752 mmHg?
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Open Question
When hydrochloric acid is poured over potassium sulfide, 42.9 mL of hydrogen sulfide gas is produced at a pressure of 752 torr and 25.8 °C. Write an equation for the gas-evolution reaction. Determine how much potassium sulfide (in grams) reacted.
Textbook Question
Consider the reaction:
2 SO2(g) + O2(g) → 2 SO3(g)
a. If 285.5 mL of SO2 reacts with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and the theoretical yield of SO3?
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