The hydrogen-filled dirigible Hindenburg had a volume of 1 . 99 × 1 0 8 L . If the hydrogen used was produced by the reaction of carbon with steam, how many kilograms of carbon would have been needed to produce enough hydrogen to fill the dirigible at 20 °C and 740 mm pressure? C ( s ) + H 2 O ( g ) → CO ( g ) + H 2 ( g )
The hydrogen-filled dirigible Hindenburg had a volume of 1 . 99 × 1 0 8 L . If the hydrogen used was produced by the reaction of carbon with steam, how many kilograms of carbon would have been needed to produce enough hydrogen to fill the dirigible at 20 °C and 740 mm pressure? C ( s ) + H 2 O ( g ) → CO ( g ) + H 2 ( g )
Solution Summary: The author explains that a balanced chemical equation follows the law of conservation of mass. The relationship between the number of reactants and product molecules is called stoichiometry.
The hydrogen-filled dirigible Hindenburg had a volume of
1
.
99
×
1
0
8 L
. If the hydrogen used was produced by the reaction of carbon with steam, how many kilograms of carbon would have been needed to produce enough hydrogen to fill the dirigible at 20 °C and 740 mm pressure?
C
(
s
)
+
H
2
O
(
g
)
→
CO
(
g
)
+
H
2
(
g
)
The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes
of nitrogen gas.
1. Write a balanced chemical equation, including physical state symbols, for the
decomposition of solid sodium azide (NaN) into solid sodium and gaseous dinitrogen.
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2. Suppose 12.0 L of dinitrogen gas are produced by this reaction, at a temperature of
13.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must
have reacted. Round your answer to 3 significant digits.
Explanation
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The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of sodium azide, which produces large volumes of nitrogen gas.
1. Write a balanced chemical equation, including physical state symbols, for the
decomposition of solid sodium azide (NaN3) into solid sodium and gaseous dinitrogen.
0
2. Suppose 25.0 L of dinitrogen gas are produced by this reaction, at a temperature of
15.0 °C and pressure of exactly 1 atm. Calculate the mass of sodium azide that must
have reacted. Round your answer to 3 significant digits.
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A hydride of silicon prepared by the reaction of Mg2Si with acid exerted a pressure of 306 torr at 26 °C in a bulb with a volume of 57.0 mL. If the mass of the hydride was 0.0861 g, what is its molecular mass? What is the molecular formula for the hydride?
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
NEET Chemistry | Group 14 Carbon Family | Theory & Problem Solving | In English | Misostudy; Author: Misostudy;https://www.youtube.com/watch?v=enOGIrcHh54;License: Standard YouTube License, CC-BY