Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas. C 2 H 2 , and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC 2 . with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons. (a) Outline the steps necessary to answer the following question: What volume of C 2 H 2 at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC 2 with water? (b) Answer the question.
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas. C 2 H 2 , and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC 2 . with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons. (a) Outline the steps necessary to answer the following question: What volume of C 2 H 2 at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC 2 with water? (b) Answer the question.
Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas.
C
2
H
2
, and solid calcium hydroxide were formed by the reaction of calcium carbide,
CaC
2
. with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons.
(a) Outline the steps necessary to answer the following question: What volume of
C
2
H
2
at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of
CaC
2
with water?
What is the equilibrium partial pressure of N9(g) at 1500°C and 1 atm total pressure?
When limestone (solid CaCO3) is heated, it decomposes into lime (solid CaO) and carbon dioxide gas. This is an extremely useful industrial process of great antiquity, because powdered lime mixed with water is the basis for mortar and concrete — the lime absorbs CO2 from the air and turns back into hard, durable limestone.
Suppose some calcium carbonate is sealed into a limekiln of volume 550.L and heated to 700.0°C. When the amount of CaCO3 has stopped changing, it is found that 4.14kg have disappeared.
Calculate the pressure equilibrium constant Kp this experiment suggests for the equilibrium between CaCO3 and CaO at 700.0°C. Round your answer to 2 significant digits.
Note for advanced students: it's possible there was some error in this experiment, and the value it suggests for Kp does not match the accepted value.
A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.
General, Organic, and Biological Chemistry (3rd Edition)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.