How much CO2 (L) is produced when 2.10 kg of sodium bicarbonate reacts with excess hydrochloric acid at 25.0 °C and 1.23 atm? A)
2 answers:
The equation representing the reaction between sodium bicarbonate and hydrochloric acid is as follows:
The substances and
combine in a 1:1 ratio. Therefore, we calculate the quantity of sodium bicarbonate and its molar mass to determine the moles formed.
.
.
We also recognize that the stoichiometric proportions are 1:1:1:1:1, which leads to the conclusion that the moles of equal 24.977 moles.
Next, we apply the ideal gas equation , where P denotes pressure, V refers to volume, R is the gas constant, and T represents the temperature in kelvins. We rearrange to solve for V
The final answer should be expressed in liters, , hence
Response: The right choice is (B)
Clarification:
Initially, we need to find the number of moles of .
Next, we will determine the moles of .
The balanced chemical equation is
From this equation, we derive that
Since 1 mole of produces 1 mole of
Thus, 25 moles of yield 25 moles of
Now we need to compute the volume of .
Utilizing the ideal gas law,
Here,
P = pressure of gas = 1.23 atm
V = volume of gas =?
T = temperature of gas =
n = number of moles of gas = 25 moles
R = gas constant = 0.0821 L.atm/mole.K
Substituting in all the known variables into the ideal gas equation results in
Consequently, the volume of carbon dioxide gas generated is
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Answer:
3.816 × 10⁻³ M
Explanation:
A stock solution of Cu²⁺(aq) is made by dissolving 0.8875 g of solid Cu(NO₃)₂∙2.5H₂O in a 100.0-mL volumetric flask, and then brought up to volume with water. What is the molarity (in M) of Cu²⁺(aq) in this stock solution?
We can derive the following relations:
- The molar mass of Cu(NO₃)₂∙2.5H₂O is 232.59 g/mol.
- Each mole of Cu(NO₃)₂∙2.5H₂O yields one mole of Cu²⁺.
The moles of Cu²⁺ present in 0.8875 g of Cu(NO₃)₂∙2.5H₂O are:
The molarity of Cu²⁺ is: