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?
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium
with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based
L-atm
on experimentally collected data, the student calculates R to equal 0.0832
mol·K
L-atm
Ideal gas law constant from literature: 0.08206
mol·K
(a) Determine the percent error for the student's R-value.
Percent error =
%
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but
does not dislodge it.
The student does not clean the zinc metal with sand paper.
The student does not equilibrate the water levels within the eudiometer and the beaker at the
end of the reaction. The water level in the eudiometer is 1-inch above the water level in the
beaker.
The student uses the barometric pressure for the lab to calculate R.
Write the balanced chemical equation for conversion of Al(s) to KAl(SO4)2·12H2O(s) in aqueous solution.
3. Hydrochloric acid is a strong acid that can be used to make sodium chloride and a weak acid, nitrous acid. Write the
balanced chemical equation of this reaction. (You can use the information in part b to help you determine states),
b. Using the information below determine the AºHrn of the gencration of nitrous acid and sodium chloride.
2NACI (s) + H;O (1) → 2HCI (aq) + Na;O (aq)
AH, = 507.1 kJ/mol
NO (g) + NO2 (g) → Na;O (aq) + 2NaNO; (aq)
AH,n = -427.4 kJ/mol
NO (g) + NO2 (g) →N20 (g) +
AHrxn = -42.8 kJ/mol
(8)
2HNO2 (aq)
→ N20 (g) + O2 (g) + H2O (I)
AHrn = 34.2 kJ/mol
General, Organic, and Biological Chemistry (3rd Edition)
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