Urgent!
Considering the following equation. Na2Co3(s)+H3Po4(s)=>Na3Po4(s)+H2O(l)+CO2(g).
a) what's the energy amount envolved in the reaction?
b)what is the volum of the released gas?
c)what the volum of the consumed phosphate acid, considering d=1,69g/ml?
Really need to sold this guys. Thank so much who could help!!!
To find the answers to the questions, we need to use stoichiometry and relevant equations. Let's go step by step:
a) To calculate the energy amount involved in the reaction, we need to know the enthalpy change (ΔH) for the reaction. This information is typically given in a chemical reaction equation or can be looked up in tables. Unfortunately, the enthalpy change is not provided in the equation you've given. Without knowing the enthalpy change, we cannot determine the energy involved in the reaction. It would be best to consult additional sources or provide more information to find the enthalpy change.
b) To determine the volume of the released gas (CO2), we need to use the ideal gas law equation: PV = nRT. However, we don't have the pressure (P), number of moles (n), or temperature (T) information. Therefore, we cannot calculate the volume of the released gas without more data.
c) To find the volume of the consumed phosphoric acid, we need to use its density (d) and its mass (m). The equation you've given does not specify the mass of H3PO4 consumed. If you have the mass, say m grams, you can use the following equation:
Volume = mass/density
Volume = m/d
where m is the mass of the consumed phosphoric acid and d is the density (1.69 g/mL according to your question). You can substitute the values into the equation to find the volume.
Remember, it is essential to provide all the necessary information, such as m (mass), P (pressure), n (number of moles), and T (temperature), to accurately calculate the desired values.