Barium reacts with H2O to produce hydrogen.
(a) Write a balanced chemical equation for the reaction, using the smallest integer coefficients possible. Write states in brackets. (Hint: Ba(OH)2 is the second product.) in the parenthesis label state also: aq, s , l , g
________ ( ) + _________( ) ------> ________( ) + ________( )
(b) Calculate the mass of pure Ba that will furnish 8.23 L of hydrogen at a pressure of 0.706 atm and a temperature of 26.6°C.
________g
a) the balanced equation is as follows
Ba(s) + 2H2O (l) -----------------------> Ba(OH)2 (aq) + H2 (g)
Ba(OH)2 is slightly soluble in water
b) volume = 8.23 L
pressure = 0.706 atm
temperature = 26.6c = 299.6 Kelvin
gas constant R = 0.0821 L atm / mol k
using the ideal gas equation PV = nRT
n = PV / RT
n = 0.706 * 8.23 / 0.0821 * 299.6 = 0.2362 moles
from the equation
1 mole Ba --------------------------> 1 mole H2
? ------------------------------------> 0.2362 moles
=> 0.2362 moles of Ba
mass of Ba = moles * molar mass = 0.2362 * 137.327 = 32.44 grams
Barium reacts with H2O to produce hydrogen. (a) Write a balanced chemical equation for the reaction,...
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