2*3.52*17
=<span>119.68 grams</span>
Answer:
2Na + 2H2O - - - > 2NaOH + H2
Explanation: This is a an exothermic reaction.
Exothermic reaction : a reaction in which heat is released during a reaction with the product
Answer:
(molecular) 3 CaCl₂(aq) + 2 (NH₄)₃PO₄(aq) ⇄ Ca₃(PO₄)₂(s) + 6 NH₄Cl(aq)
(ionic) 3 Ca²⁺(aq) + 6 Cl⁻(aq) + 6 NH₄⁺(aq) + 2 PO₄³⁻(aq) ⇄ Ca₃(PO₄)₂(s) + 6 NH₄⁺(aq) + 6 Cl⁻(aq)
(net ionic) 3 Ca²⁺(aq) + 2 PO₄³⁻(aq) ⇄ Ca₃(PO₄)₂(s)
Explanation:
The molecular equation includes al the species in the molecular form.
3 CaCl₂(aq) + 2 (NH₄)₃PO₄(aq) ⇄ Ca₃(PO₄)₂(s) + 6 NH₄Cl(aq)
The ionic equation includes all the ions (species that dissociate in water) and the species that do not dissociate in water.
3 Ca²⁺(aq) + 6 Cl⁻(aq) + 6 NH₄⁺(aq) + 2 PO₄³⁻(aq) ⇄ Ca₃(PO₄)₂(s) + 6 NH₄⁺(aq) + 6 Cl⁻(aq)
The net ionic equation includes only the ions that participate in the reaction and the species that do not dissociate in water. In does not include <em>spectator ions</em>.
3 Ca²⁺(aq) + 2 PO₄³⁻(aq) ⇄ Ca₃(PO₄)₂(s)
Answer:
Total pressure in flask is 2.37 atm.
Explanation:
According to the Dalton's law of partial pressure, the total pressure of the flask would be the sum of partial pressure of the gases present in mixture.
P(total) = P1+ P2+P3+...Pn
n= number of gases present
Given data:
Pressure of argon gas = 0.72 atm
Pressure of oxygen gas = 1.65 atm
Total pressure in flask = ?
Solution:
P(total) = P (argon) + P (oxygen)
P(total) = 0.72 + 1.65
P(total) = 2.37 atm
