Given the following balanced reaction: 2 NH3 +CO2 --> CH4N2O + H2O A reaction produces 87.5g of CH4N2O upon the reaction of 6
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There are 34 g of oxygen in the container.
We can use the<em> Ideal Gas Law</em> to solve this problem.
But , so
and
STP is 0 °C and 1 bar, so
<u>Answer:</u> The mass of water that should be added in 203.07 grams
<u>Explanation:</u>
To calculate the molality of solution, we use the equation:
Where,
m = molality of barium iodide solution = 0.175 m
= Given mass of solute (barium iodide) = 13.9 g
= Molar mass of solute (barium iodide) = 391.14 g/mol
= Mass of solvent (water) = ? g
Putting values in above equation, we get:
Hence, the mass of water that should be added in 203.07 grams