I can't answer this question without knowing what the specific heat capacity of the calorimeter is. Luckily, I found a similar problem from another website which is shown in the attached picture.
Q = nCpΔT
Q = (1.14 g)(1 mol/114 g)(6.97 kJ/kmol·°C)(10°C)(1000 mol/1 kmol)
<em>Q = +6970 kJ</em>
When there is change of state solid to liquid to gas or in any order then there will be change in intermolecular bonds. amount of intermolecular bonds.
Answer:
Heating this gas to 55 °C will raise its volume to 6.87 liters.
Assumption: this gas is ideal.
Explanation:
By Charles's Law, under constant pressure the volume of an ideal gas is proportional to its absolute temperature (the one in degrees Kelvins.)
Alternatively, consider the ideal gas law:
.
- is the number of moles of particles in this gas. should be constant as long as the container does not leak.
- is the ideal gas constant.
- is the pressure on the gas. The question states that the pressure on this gas is constant.
Therefore the volume of the gas is proportional to its absolute temperature.
Either way,
.
.
For the gas in this question:
- Initial volume: .
Convert the two temperatures to degrees Kelvins:
- Initial temperature: .
- Final temperature: .
Apply Charles's Law:
.
The answer is B because that is how plants give off oxygen.
A solvent is a liquid that dissolves a solid, liquid or gaseous solute. A solute is a substance dissolved in another substance. A solute and a solvent make up a solution.
the mass of the solution = mass of solvent (water) + mass of solute (NaCl)
the mass of the solution = 217 grams + 17.8 grams = 234.8 grams
Note:
according to the solubility of sodium chloride which given in the question 360 g/dm3 all the amount of NaCl added to water was totally dissolved.