Answer:
29260J
Explanation:
Given parameters:
Mass of water sample = 100g
Initial temperature = 30°C
Final temperature = 100°C
Unknown:
Energy required for the temperature change = ?
Solution:
The amount of heat required for this temperature change can be derived from the expression below;
H = m c (ΔT)
H is the amount of heat energy
m is the mass
c is the specific heat capacity of water = 4.18J/g°C
ΔT is the change in temperature
Now insert the parameters and solve;
H = 100 x 4.18 x (100 - 30)
H = 100 x 4.18 x 70 = 29260J
The correct answer to this question would be heat energy
Answer:
compounds , because they're combined
Answer is: molar mass
of compound is 154,58 g/mol.<span>
m(</span>naphthalene<span>) = 10 g = 0,01 kg.
m(unknown compound) = 1,00 g.
</span>Δ<span>T (solution) = 4,47 °C.
Kf(</span>naphthalene) = 6,91°C/m<span>; cryoscopic
constant.
M</span>(unknown compound) = Kf(naphthalene)· m(unknown compound) ÷
m(naphthalene)<span> · ΔT(solution).
M(xylene) = </span>6,91°C/m<span> · 1 g ÷ 0,01 kg · 4,47</span>°C<span>.
M(xylene) = 154,58 g/mol.</span>
The pressure of the xenon gas will increase if the number of moles increases because as more molecules are in the container, the molecules hit the container of the wall more often (option C).
<h3>What is an ideal gas?</h3>
Ideal gas is a hypothetical gas, whose molecules exhibit no interaction, and undergo elastic collision with each other and with the walls of the container.
According to this question, a 1.81 mol sample of Xenon gas is confined in a 42.6 liter container at 14.1 °C. If the amount of gas is increased to 2.72 mol, holding the volume and temperature constant, the pressure will increase.
An increase in the number of gas molecules, while container volume stays constant causes the pressure to increase due to the fact that the molecules will collide more with the walls of the container.
Learn more about ideal gases at: brainly.com/question/28257995
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