Answer:
2407 kJ/mol
Explanation:
Given:
Mass of water = 40.00 kg
= 1.065 °C
Net Heat transfer during heating:
Specific heat of water = 4.187 kJ/kg°C
Q = 178.3662 kJ
Heat gained by water is heat lost by the compound. Thus, heat lost = 178.3662 kJ
Also,
Mass = 4.000 g
Molar mass of 
The formula for the calculation of moles is shown below:
Thus,
<u>Standard heat of formation = 178.3662 kJ / 0.0741 mol=2407 kJ/mol (In correct significant digits)</u>
The answer would be 6.023 x 10E23
E= exponent
Answer:
Ice melts into liquid water- endothermic
A process with a calculated positive q - endothermic
Wood burns in a fireplace - exothermic
A process with a calculated negative q - exothermic
Acid and base are mixed, making test tube feel hot - exothermic
Solid dissolves into solution, making ice pack feel cold - endothermic
Explanation:
An endothermic process is one in which heat is absorbed from the surroundings. The absorption of heat means that heat is removed from the surroundings hence the surroundings feel cool. When heat is absorbed, q is positive.
An exothermic process is one in which heat is released to the surroundings. The evolution of heat means that heat is released into the surroundings hence the surroundings feel hot . When heat is evolved, q is negative.
If the force is applied to lift the box, then there is no work done as the displacement of the box is not in the same direction of the box.
However, if the force is being applied to move the box in the direction of the force, then the work done is:
Work = force x distance
Work = 1500 x 3
Work = 4,500 Joules
