Molarity is expressed as moles/L, where L stands for the total volume of the solution. Accordingly, if I have a 1M solution of NaCl, I really have slightly less than 1L of water since the NaCl makes up the remaining solution to give it a FINAL volume of 1L. However, molality is measured in moles per kilogram of the solvent. This implies that I would add 1mol of NaCl to 1kg of water to get a 1 molal solution (the solvent). This occurs to be 1L of water because of the density of water. Due to the addition of some NaCl to my 1kg of water, the final solution volume in this instance is a little bit more than 1L. In terms of temperature, your final volume of 1L of solution would vary if you heated the 1 MOLAR solution from the first paragraph. Due to the expansion caused by heating, it will get bigger. As a result, the molarity varies when the same amount of NaCl is dissolved in more solution. However, the water will expand but not change in mass when the 1 MOLAL solution is heated. There will still be 1 kilogram of water even after expansion. Because of this, regardless of the temperature, the same quantity of NaCl is dissolved in the same mass of solute.
Answer:
54g of water
Explanation:
Based on the reaction, 1 mole of methane produce 2 moles of water.
To solve this question we must find the molar mass of methane in order to find the moles of methane added. With the moles of methane and the chemical equation we can find the moles of water produced and its mass:
<em>Molar mass CH₄:</em>
1C = 12g/mol*1
4H = 1g/mol*4
12g/mol + 4g/mol = 16g/mol
<em>Moles methane: </em>
24g CH₄ * (1mol / 16g) = 1.5 moles methane
<em>Moles water:</em>
1.5moles CH₄ * (2mol H₂O / 1mol CH₄) = 3.0moles H₂O
<em>Molar mass water:</em>
2H = 1g/mol*2
1O = 16g/mol*1
2g/mol + 16g/mol = 18g/mol
<em>Mass water:</em>
3.0moles H₂O * (18g / mol) =
<h3>54g of water</h3>
Answer:
hope it is use full to you
Explanation:
The gas constant is denoted by the symbol R or R. It is equivalent to the Boltzmann constant, but expressed in units of energy per temperature increment per mole, i.e. the pressure–volume product, rather than energy per temperature increment per particle.
it is a physical constant that is featured in many fundamental equations in the physical sciences, such as the ideal gas law, the Arrhenius equation, and the Nernst equation. As a consequence, the value of the gas constant is also exactly defined.