Answer:
ΔHrxn = - 1534.3 J
Explanation:
Given the assumptions and the formula for the change in enthalpy:
ΔHrxn = m x C x ΔT, where
m is the mass of solution given 135.4 g
C is the heat capacity 4.2 J/g .K and,
ΔT is the change in temperature
we have ,
T₁ = ( 18.1 + 273) K = 291.1 K
T₂ = ( 15.4 +273) K = 288.4 K
ΔHrxn = 135.3 g x 4.2 J/gK x ( 288.4 -291.1 ) K = - 1534.3 J
After verifying our result has the correct unit, the answer is -1534.3 Joules, and the negative sign tells us it is an endothermic reaction decreasing the final temperature.
Answer:
The electric force between them decreases
Explanation:
The force between two charged particle is given by :
Where
r is the distance between charges
If the distance between the charges is increased, the electric force gets decreased as there is an inverse relation between force and distance.
Hence, the correct option is (c) "The electric force between them decreases"
Answer:
0.92 kg
Explanation:
The volume occupied by the air is:
The moles of air are:
The heat required to heat the air by 10.0 °C (or 10.0 K) is:
Methane's heat of combustion is 55.5 MJ/kg. The mass of methane required to heat the air is:
Answer:
No effect will be observed.
Explanation:
Let's consider the following reaction at equilibrium.
CuS(s) + O₂(g) ↔ Cu(s) + SO₂(g)
To assess the effect of increasing the pressure, we need to consider Le Chatelier's Principle: if a system at equilibrium suffers a perturbation, it will shift its equilibrium to counteract the effect of such perturbation.
According to the ideal gas equation, the pressure of a gas is proportional to the number of moles. If we increase the temperature, the system will try to reduce it by shifting the equilibrium towards the side with less gaseous moles. However, in this reaction, we have the same number on gaseous moles on the left side and on the right side (1 mole). As a consequence, the increase in the temperature will have no effect on the equilibrium.
