Given 4.68L CO2 and the following unbalanced equation, complete a-h. ___CaCO3 (s) + ___HCl (aq) → ___CO2 (g) + ___H2O (l) + ___CaCl2 (s) a) Balance the equation density of CO2 = 1.96 g/L (1.96g CO2/ 1L CO2) b) __?__ g CO2 produced (this is the theoretical yield of g CO2) c) __?__ mol CO2 produced (this is the theoretical yield of mol CO2)
Given 4.68L CO2 and the following unbalanced equation, complete a-h.
___CaCO3 (s) + ___HCl (aq) → ___CO2 (g) + ___H2O (l) + ___CaCl2 (s)
a) Balance the equation
density of CO2 = 1.96 g/L (1.96g CO2/ 1L CO2)
b) __?__ g CO2 produced (this is the theoretical yield of g CO2)
c) __?__ mol CO2 produced (this is the theoretical yield of mol CO2)
d) __?__ mol HCl produced (this is the theoretical yield of mol HCl)
e) __?__ g HCl produced (this is the theoretical yield of grams HCl)
f) __?__ mol CaCO3 produced (this is the theoretical yield of mol CaCO3)
g) __?__ g CaCO3 produced (this is the theoretical yield of g CaCO3)
h) What is the actual yield of L CO2, given 85% yield?
Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.
The reaction taking place is given as,
=> CaCO3 (s) + HCl (aq) -------> CO2 (g) + H2O (l) + CaCl2 (s)
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